How atomic radius is defined, and trends across a period and down a group. Created by Jay. Watch the next lesson: https://www.khanacademy.org/science/chemistry/periodic-table/periodic-table-trends-bonding/v/atomic-and-ionic-radii?utm_source=YT&utm_medium=Desc&utm_campaign=chemistry Missed the previous lesson? https://www.khanacademy.org/science/chemistry/periodic-table/copy-of-periodic-table-of-elements/v/periodic-table-valence-electrons?utm_source=YT&utm_medium=Desc&utm_campaign=chemistry Chemistry on Khan Academy: Did you know that everything is made out of chemicals? Chemistry is the study of matter: its composition, properties, and reactivity. This material roughly covers a first-year high school or college course, and a good understanding of algebra is helpful. About Khan Academy: Khan Academy offers practice exercises, instructional videos, and a personalized learning dashboard that empower learners to study at their own pace in and outside of the classroom. We tackle math, science, computer programming, history, art history, economics, and more. Our math missions guide learners from kindergarten to calculus using state-of-the-art, adaptive technology that identifies strengths and learning gaps. We've also partnered with institutions like NASA, The Museum of Modern Art, The California Academy of Sciences, and MIT to offer specialized content. For free. For everyone. Forever. #YouCanLearnAnything Subscribe to Khan Academy’s Chemistry channel: https://www.youtube.com/channel/UCyEot66LrwWFEMONvrIBh3A?sub_confirmation=1 Subscribe to Khan Academy: https://www.youtube.com/subscription_center?add_user=khanacademy
Views: 479936 Khan Academy
This chemistry video tutorial provides a basic introduction into atomic radius which is one of the four main periodic table trends you need to know. Atomic radius increases as you down a group and to the left across the periodic table. Atomic radius decreases with effective nuclear charge but increases with each successive energy level added to an atom as you go down a group. New Chemistry Video Playlist: https://www.youtube.com/watch?v=bka20Q9TN6M&t=25s&list=PL0o_zxa4K1BWziAvOKdqsMFSB_MyyLAqS&index=1 Access to Premium Videos: https://www.patreon.com/MathScienceTutor Facebook: https://www.facebook.com/MathScienceTutoring/
Views: 19264 The Organic Chemistry Tutor
This chemistry video tutorial focuses on periodic trends such as ionic radius and atomic radius. It provides plenty of examples and explains the fundamental concepts of why some ions are smaller than atoms while others are larger. Here is a list of topics 1. Atomic Radii decreases left to right 2. Effective Nuclear Charge, Atomic Number, and Number of Protons 3. Atomic Radius Increases from top to bottom in the periodic table due to additional energy levels 4. Neutral vs Positively Charged Ion / Cation – Number of Shells or Energy Levels 5. Neutral Parent Atom vs Negatively Charged Ion / Anion – Electron Repulsion & Electron Cloud Expansion 6. General Ionic Radii Trend – Cations are smaller than Anions
Views: 47296 The Organic Chemistry Tutor
Why is the periodic table arranged the way it is? There are specific reasons, you know. Because of the way we organize the elements, there are special patterns that emerge. And you know how Professor Dave feels about patterns. He likes them. Subscribe: http://bit.ly/ProfDaveSubscribe [email protected] http://patreon.com/ProfessorDaveExplains http://professordaveexplains.com http://facebook.com/ProfessorDaveExpl... http://twitter.com/DaveExplains General Chemistry Tutorials: http://bit.ly/ProfDaveGenChem Organic Chemistry Tutorials: http://bit.ly/ProfDaveOrgChem Biochemistry Tutorials: http://bit.ly/ProfDaveBiochem Classical Physics Tutorials: http://bit.ly/ProfDavePhysics1 Modern Physics Tutorials: http://bit.ly/ProfDavePhysics2 Mathematics Tutorials: http://bit.ly/ProfDaveMaths Biology Tutorials: http://bit.ly/ProfDaveBio American History Tutorials: http://bit.ly/ProfDaveAmericanHistory
Views: 922974 Professor Dave Explains
* Atoms further down the periodic table are larger because they have more shells of electrons * Atoms farther to the right on the table are smaller because they have the same number of shells but more protons * Johnny was a scientist, but Johnny is no more, what Johnny thought was H2O was C4H7Cl2PO4 Check me out: http://www.chemistnate.com
Views: 9872 chemistNATE
This chemistry video tutorial provides a basic introduction into the periodic trends of the ionic radius of ions. It explains how to rank in order of increasing ionic radii - the sizes of isoelectric ions - which are ions that have the same number of electrons and the same electron configuration. Anions are usually bigger than cations. New Chemistry Video Playlist: https://www.youtube.com/watch?v=bka20Q9TN6M&t=25s&list=PL0o_zxa4K1BWziAvOKdqsMFSB_MyyLAqS&index=1 Access to Premium Videos: https://www.patreon.com/MathScienceTutor Facebook: https://www.facebook.com/MathScienceTutoring/
Views: 23412 The Organic Chemistry Tutor
* Helium (He) is the smallest atom on the periodic table * Francium (Fr) is the largest. * As you move down the table, you add electron shells, so the atoms get bigger. * As you move right, you add protons (and not electron shells), so the atoms get smaller. * What do you do with a dead chemist? Dissolve him in HF and never speak of it again. Check me out: http://www.chemistnate.com
Views: 7193 chemistNATE
This chemistry video tutorial explains the concepts of periodic trends such as first ionization energy, electron affinity, atomic radius, and ionic radii, electronegativity and metallic character. It contains plenty of examples and practice problems. Here is a list of topics: 1. Periodic Trends - Atomic Size 2. Atomic Radii - Effective Nuclear Charging - Adding Protons to Increase The Charge of the Nucleus 3. Inner Core Electrons vs Outer Valence Electrons 4. Atomic Radius Increases from left to right 5. Atomic Radii Increases from top to bottom on the periodic table 6. Shielding Effect and Electron Repulsion 7. Coulomb's Law Equation / Formula - Relationship Between Electrostatic Force, Distance, and Charge - like charges repel and opposite charges attract. 8. Ionic Radii Trend - Cations vs Anions 9. Positively Charged Ions are Smaller Than Parent Neutral Atom 10. Negatively Charged Ions are Larger Than Parent Atom 11. How to calculate the number of electrons in an atom or ion 12. Principal quantum number and number of shells - atomic size 13. How to rank the elements in order of increasing atomic radii 14. how to rank isoelectronic ions in decreasing order of atomic / ionic size 15. isoelectronic species - same electron configuration 16. Metallic Character Trend - Metals vs Nonmetals 17. Electronegativity Trend - The ability of an atom to attract an electron to itself - increases toward fluorine 18. Electronegative Nonmetals vs Electropositive Metals 19. First Ionization Energy Trend - Increases left to right and bottom to top across a group 20. Ionization Energy - Energy required to remove an electron from a gaseous atom 21. First Ionization Energy vs Second Ionization Energy 22. Jump in Ionization Energy - Number of Valence Electrons 23. Ionization Energy Exceptions - Paired vs Unpaired Electrons in 2s and 2p orbitals 24. Electron Affinity Trend - The Energy change associated with the addition of an electron to a gaseous atom 25. Exothermic vs Endothermic Electron Affinity Processes 26. Half Filled vs Empty S and p orbitals 27.
Views: 79724 The Organic Chemistry Tutor
All hail RADIUS! If you want to understand why an atom does what it does, take a look at those outermost electrons (a.k.a. the valence electrons). You can look at how many there are, but you can also look at how far away from the nucleus they are. Let's show the periodic trends for that. Quick visual of radius: http://youtu.be/ba2yN2HtPTA Another one: http://youtu.be/VopLrkfXfGw
Views: 1276 Guillotined Chemistry
To support me in my journey you can donate ([email protected] 9161123482) or Alakh Pandey ,Bank of Baroda, Rajrooppur, Allahabad,U.P IFSC: BARB0RAJROO Account No: 19210100020819 A small amount of Rs 100 even will be of great help. Follow us on: Instagram https://www.instagram.com/physicswallah/ Facebook: https://www.facebook.com/physicswallah Class 11 chap 3 | Periodic Table 01 | Historical Development | Periodic Classification Of Elements | https://youtu.be/TOXF8LXEFJw Class 11 chap 3 | Periodic Table 02 | Modern Periodic Table | Periodic Classification Of Elements | https://youtu.be/ZXpCDByQPdA 11 chap 3 | Periodic Table 03 || How to Find Group, Period and Block of any Element || spdf trick https://youtu.be/V7BL9HKZYMY Class 11 chap 3 | Periodic Table 04 || Atomic Radius ,Ionic Radius its Variation || JEE MAINS /NEET https://youtu.be/hGaKK3XrMJQ 11 chap 3 | Periodi c Table 05 | Ionisation Energy | Ionisation Energy IIT Ionisation Potential IIT https://youtu.be/6HqlknZbqJI 11 chap 3 | Periodic Table 06 | Electron Affinity IIT JEE NEET | Electron Gain Enthalpy IIT JEE NEET https://youtu.be/O6ToralUhKE 11 chap 3 | Periodic Table 07||Electronegativity IIT JEE || Electronegativity NEET || https://youtu.be/WmO3uCp23b4
Views: 281336 Physics Wallah - Alakh Pandey
Periodic Trends | Determine which atom has the smallest atomic radii (radius) | Chemistry | Whitwell High School | UTC - University of Tennessee at Chattanooga www.whitwellhigh.com Instructor/Professor: Johnny Cantrell
Views: 25403 Johnny Cantrell
The size of an ion can be determined by: * How many shells have electrons in them. More shells = larger ion * How many protons the ion has. More protons = smaller ion * How many electrons the ion has. All else being equal, more electrons = larger ion. * Metal ions (positive, cations) are smaller than their corresponding elements * Non-metal ions (negative, anions) are larger than their corresponding elements. Check me out: http://www.chemistnate.com
Views: 12118 chemistNATE
DeltaStep is a social initiative by graduates of IIM-Ahmedabad, IIM-Bangalore, IIT-Kharagpur, ISI-Kolkata, Columbia University (USA), NTU (Singapore) and other leading institutes. At DeltaStep, we understand that just like every child has a unique face, a unique fingerprint; he has a unique learning ability as well. Hence we have built an intelligent adaptive learning system that delivers a tailor-made learning solution and helps a student to learn at his own pace because when it comes to learning, one size does not fit all. Learn from 1000s of such interesting videos, practice from more than 1,00,000 questions, learn complex concepts through games, take timed tests, get detailed reports & in-depth analysis even via SMS and Whatsapp and many more amazing features. Class wise mapping available for all leading boards including ICSE and CBSE. Create your personal learning account. Register for FREE at www.deltastep.com.
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✔ https://StudyForce.com ✔ https://Biology-Forums.com ✔ Ask questions here: https://Biology-Forums.com/index.php?board=33.0 Follow us: ▶ Facebook: https://facebook.com/StudyForcePS/ ▶ Instagram: https://instagram.com/studyforceonline/ ▶ Twitter: https://twitter.com/studyforceps Q1. On the basis of periodic trends, choose the larger atom from each pair (if possible). Explain your choices. (a) N or F (b) C or Ge (c) N or Al (d) Al or Ge Q2. On the basis of periodic trends, choose the larger atom from each pair (if possible): (a) Sn or I (b) Ge or Po (c) Cr or W (d) F or Se Q3. Arrange these elements in order of decreasing radius: S, Ca, F, Rb, Si. N atoms are larger than F atoms because, as you trace the path between N and F on the periodic table, you move to the right within the same period (row). As you move to the right across a row, the effective nuclear charge experienced by the outermost electrons increases, resulting in a smaller radius. Ge atoms are larger than C atoms because, as you trace the path between C and Ge on the periodic table, you move down a column. Atomic size increases as you move down a column because the outermost electrons occupy orbitals with a higher principal quantum number that are therefore larger, resulting in a larger atom. Al atoms are larger than N atoms because, as you trace the path between N and Al on the periodic table, you move down a column (atomic size increases) and then to the left across a row (atomic size increases). These effects add together for an overall increase. Based on periodic trends alone, you cannot tell which atom is larger, because as you trace the path between Al and Ge you go to the right across a row (atomic size decreases) and then down a column (atomic size increases). These effects tend to oppose each other, and it is not straightforward to tell which one dominates.
Views: 59 Study Force
Get your free Ultimate Chemistry Cheat Sheet here: https://www.chemin10.com/optin?ims=jemvs&utm_source=YT+Periodic+Table Isoelectronic Series Atomic Radius An isoelectronic series is a series of elements and ions that have equal numbers of electrons. Since they each have the same number of electrons, their periodic trend in atomic radius and ionic radius predicts that the isoelectronic species with the greatest number of protons will have the smallest radius. This is because, according to Coulomb's law, the larger nuclear charge of the species with the greatest number of protons results in an increase in the attraction between between the nucleus and its outermost electrons. This increase in the attractive force brings the outermost electrons in closer to the nucleus, resulting in a smaller radius. Today's chemistry question of the day: Which of the following has the largest radius? A. Sr2+ B. Rb+ C. Kr D. Br- E. Se2- Join us at http://chemin10.com to receive the Chemistry Question of the Day delivered to your inbox, as well as more videos and an online chemistry community of like-minded chemistry students! https://youtu.be/QOKVAAc2MN8 isoelectronic series isoelectronic species isoelectronic species radius isoelectronic species atomic radius isoelectronic species ionic radius isoelectronic series size isoelectronic series atomic radius
Views: 20005 CheminTen
What are the periodic trends? Electronegativity, Atomic Radius, Ionization Energy, and Electron Affinity. How to remember them? F has the highest electronegativity, electron affinity, and one of the largest ionization energies. It is also one of the smallest atoms.
Views: 272586 chemistNATE
Explaining group and period trends in atomic and ionic radii. Created by Jay. Watch the next lesson: https://www.khanacademy.org/test-prep/mcat/physical-processes/periodic-table-of-elements/v/group-trend-for-ionization-energy?utm_source=YT&utm_medium=Desc&utm_campaign=mcat Missed the previous lesson? https://www.khanacademy.org/test-prep/mcat/physical-processes/periodic-table-of-elements/v/periodic-table-valence-electrons?utm_source=YT&utm_medium=Desc&utm_campaign=mcat MCAT on Khan Academy: Go ahead and practice some passage-based questions! About Khan Academy: Khan Academy offers practice exercises, instructional videos, and a personalized learning dashboard that empower learners to study at their own pace in and outside of the classroom. We tackle math, science, computer programming, history, art history, economics, and more. Our math missions guide learners from kindergarten to calculus using state-of-the-art, adaptive technology that identifies strengths and learning gaps. We've also partnered with institutions like NASA, The Museum of Modern Art, The California Academy of Sciences, and MIT to offer specialized content. For free. For everyone. Forever. #YouCanLearnAnything Subscribe to Khan Academy’s MCAT channel: https://www.youtube.com/channel/UCDkK5wqSuwDlJ3_nl3rgdiQ?sub_confirmation=1 Subscribe to Khan Academy: https://www.youtube.com/subscription_center?add_user=khanacademy
Views: 44449 Khan Academy Organic Chemistry
Atomic radius: 1:35 Ionic radius: 2:22 Electronegativity: 3:58 1st Ionization Energy: 5:03 Melting Point: 6:11 Reactivity: 11:02 Summary: 12:58 Contact me! :) Facebook: https://facebook.com/theoery
Views: 7336 Theo K.
Part 2 in our series of periodic trends, here Darth Vader explains why atomic radius decreases across a period and increases down a group. While moving across a period, the # of protons is increasing, while shielding increases very little (sometimes we ignore the change). The energy level (n) remains constant and so we are basically seeing an increase in force on the valence electrons pulling them with greater force towards the nucleus. This causes the size of the atom to decrease in spite of adding matter. This can be simplified down by using effective nuclear charge (Zeff) which combines the attractions of the nucleus and the repulsions of other electrons into a single term. The effective nuclear charge increases across a period. Down a group the shielding increases and the # of protons increase. The net effect is minimal from these two changes as they act in opposition. The effective nuclear charge is constant within a group. Thus the major contributor to size changes is the change in principal quantum number (n) or energy levels occupied. Higher energy levels put electrons at greater distances from the nucleus and thus the atoms get larger down a group.
Views: 854 Scott Milam
In this video, I discuss atomic size / atomic radius – what it is, how it’s measured, and, of course, the trend for atomic size / atomic radius up, down, and across the periodic table. Atomic radius (and thus, atomic size) increases down and to the left on the periodic table. The reason it increases down a group is because of increases in the Principal Quantum Number (n), as that means there are more shells of electrons. Further, as more and more shells of electrons are added, electron shielding occurs, in which inner electrons repel outer electrons out further away from the positively charged nucleus that the outer electrons are attracted to. This results in the atom being bigger. The reason atomic size decreases to the right on the periodic table is due to increases in Effective Nuclear Charge (Zeff). As the number of protons increases, the actual nuclear charge increases, and because within a period, we’re discussing the same energy level, there is only a very slight increase in shielding with each additional electron. Thus, the effective nuclear charge, being higher, can draw in electrons more, making the atom smaller. For a suggested viewing order of the videos, information on tutoring, personalized video solutions, and an opportunity to support Moof University financially, visit MoofUniversity.com, and follow Moof University on the different social media platforms. Don't forget to LIKE, COMMENT, and SUBSCRIBE: http://www.youtube.com/subscription_center?add_user=MoofUniversity SUPPORT MOOF UNIVERSITY: http://www.moofuniversity.com/support-moof/ BUY A T-SHIRT https://shop.spreadshirt.com/moofuniversity/ INFORMATION ABOUT TUTORING AND PERSONALIZED VIDEO SOLUTIONS: http://www.moofuniversity.com/tutoring/ INSTAGRAM: https://instagram.com/moofuniversity/ FACEBOOK: https://www.facebook.com/pages/Moof-University/1554858934727545 TWITTER: https://twitter.com/moofuniversity
Views: 684 Moof University
Periodic Trends are patterns present in the periodic table based on an element's size and electron distribution. Atomic radius is defined as half the distance between the nuclei in a molecule of two identical elements. Watch more of this topic at ► http://bit.ly/28KSlJf Download this PDF: http://bit.ly/1ZWNPl1 GET MORE CLUTCH! VISIT our website for more of the help you need: http://bit.ly/28KRPuL SUBSCRIBE for new videos: http://cltch.us/1axA33X --- LET'S CONNECT! Facebook: http://cltch.us/1JLgiSZ Twitter: http://cltch.us/1NLcKpu Instagram: http://cltch.us/1If5pb7 Google+: http://cltch.us/1E34o85 Clutch Prep = Textbook specific videos to help you pass your toughest science classes.
Views: 6815 Clutch Prep
Atomic size is measured in terms of Atomic radius. Learn the trend in Atomic Radius. This is a sub-topic in the Chemistry Section of IIT JEE. This video covers Measuring Atomic Radius, Covalent Radius, Metallic Radius and Vander Valls Radius. It is a part of our IIT JEE video lecture series by Rajiv Sir - Ex Head Faculty at premier institutes for IIT JEE preparation - Resonance and Narayana. Rajiv qualified with a B.E. from IIT Bombay and has over 10 years of IIT JEE coaching experience. For more such helpful videos on IIT JEE Exam subscribe to our Channel. To know more kindly go on this link- https://goo.gl/Kzjptk You can also visit us on our website – www.ufaber.com
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The atomic radius of a chemical element is a measure of the size of its atoms, usually the mean or typical distance from the nucleus to the boundary of the surrounding cloud of electrons. Since the boundary is not a well-defined physical entity, there are various non-equivalent definitions of atomic radius.
Views: 8957 smartschoolonline
In this video, I define Ionic Size in terms of the Ionic Radius and how to determine size difference between ions and parent atoms, as well as between ions and other ions. There isn’t exactly an entirely new trend for Ionic Size / Ionic Radius. All we need to do is learn how certain ions relate in size to their parent atoms, and then apply that knowledge and understanding to what we already know and understanding about the trend for atomic size / atomic radius. Cations, when compared to their parent atoms, are SMALLER. The reason why is because cations are the result of the loss of electrons. Less electrons means less shielding, which means a higher effective nuclear charge that can draw remaining electrons closer to the nucleus, making cations smaller in size than their parent atoms. As an example, Na+ (a cation) is smaller than its parent atom, Na. Anions, when compared to their parent atoms, are BIGGER. The reason why is because anions are the result of the gaining of electrons. More electrons means more shielding, which means a lower effective nuclear charge that cannot draw remaining electrons in as close to the nucleus, making anions larger in size than their parent atoms. As an example, Cl- (an anion) is bigger than its parent atom, Cl. In the video, I go through three example problems ranking ions/atoms according to their sizes. Don't forget to LIKE, COMMENT, and SUBSCRIBE: http://www.youtube.com/subscription_center?add_user=MoofUniversity SUPPORT MOOF UNIVERSITY: http://www.moofuniversity.com/support-moof/ BUY A T-SHIRT https://shop.spreadshirt.com/moofuniversity/ INFORMATION ABOUT TUTORING AND PERSONALIZED VIDEO SOLUTIONS: http://www.moofuniversity.com/tutoring/ INSTAGRAM: https://instagram.com/moofuniversity/ FACEBOOK: https://www.facebook.com/pages/Moof-University/1554858934727545 TWITTER: https://twitter.com/moofuniversity
Views: 1002 Moof University
Description of why atomic and ionic radii vary, the trends for the variance, examples of ranking both atoms and ions by radius. Visit my Curious Learning Lessons for Lessons with embedded questions: https://curious.com/drholton/intro-to-radioactive-decay-processes/in/introduction-to-nuclear-chemistry?ref=z3PRYqMsD1Q
Views: 8280 Dr. Holton's Chemistry Channel
when you move from top to bottom in periodic table the atomic size and atomic radii increases this is because:. atomic size and atomic radii in the periodic table. Atomic radius patterns are observed throughout the periodic table. Atomic size gradually decreases from left to right across a period of elements. This is because, within a period or family of elements, all electrons are added to the same shell. Periodic trends are specific patterns that are present in the periodic table that illustrate different aspects of a certain element, including its size and its electronic properties. Major periodic trends include: electronegativity, ionization energy, electron affinity, atomic radius, melting point, and metallic character. Periodic trends, arising from the arrangement of the periodic table, provide chemists with an invaluable tool to quickly predict an element's properties. These trends exist because of the similar atomic structure of the elements within their respective group families or periods, and because of the periodic nature of the elements. Electronegativity Trends Electronegativity can be understood as a chemical property describing an atom's ability to attract and bind with electrons. Because electronegativity is a qualitative property, there is no standardized method for calculating electronegativity. However, the most common scale for quantifying electronegativity is the Pauling scale (Table A2), named after the chemist Linus Pauling. The numbers assigned by the Pauling scale are dimensionless due to the qualitative nature of electronegativity. Electronegativity values for each element can be found on certain periodic tables. An example is provided below. Electronegativity measures an atom's tendency to attract and form bonds with electrons. This property exists due to the electronic configuration of atoms. Most atoms follow the octet rule (having the valence, or outer, shell comprise of 8 electrons). Because elements on the left side of the periodic table have less than a half-full valence shell, the energy required to gain electrons is significantly higher compared with the energy required to lose electrons. As a result, the elements on the left side of the periodic table generally lose electrons when forming bonds. Conversely, elements on the right side of the periodic table are more energy-efficient in gaining electrons to create a complete valence shell of 8 electrons. The nature of electronegativity is effectively described thus: the more inclined an atom is to gain electrons, the more likely that atom will pull electrons toward itself. Ionization Energy Trends Ionization energy is the energy required to remove an electron from a neutral atom in its gaseous phase. Conceptually, ionization energy is the opposite of electronegativity. The lower this energy is, the more readily the atom becomes a cation. Therefore, the higher this energy is, the more unlikely it is the atom becomes a cation. Generally, elements on the right side of the periodic table have a higher ionization energy because their valence shell is nearly filled. Elements on the left side of the periodic table have low ionization energies because of their willingness to lose electrons and become cations. Thus, ionization energy increases from left to right on the periodic table. Another factor that affects ionization energy is electron shielding. Electron shielding describes the ability of an atom's inner electrons to shield its positively-charged nucleus from its valence electrons. When moving to the right of a period, the number of electrons increases and the strength of shielding increases. As a result, it is easier for valence shell electrons to ionize, and thus the ionization energy decreases down a group. Electron shielding is also known as screening. Electron Affinity Trends As the name suggests, electron affinity is the ability of an atom to accept an electron. Unlike electronegativity, electron affinity is a quantitative measurement of the energy change that occurs when an electron is added to a neutral gas atom. The more negative the electron affinity value, the higher an atom's affinity for electrons. Electron affinity generally decreases down a group of elements because each atom is larger than the atom above it (this is the atomic radius trend, discussed below). This means that an added electron is further away from the atom's nucleus compared with its position in the smaller atom. With a larger distance between the negatively-charged electron and the positively-charged nucleus, the force of attraction is relatively weaker. Therefore, electron affinity decreases. Moving from left to right across a period, atoms become smaller as the forces of attraction become stronger. This causes the electron to move closer to the nucleus, thus increasing the electron affinity from left to right across a period for more ? Facebook:https://www.facebook.com/bakedofcakes/ ? Twitter: https://twitter.com/MudasarQazi7
Views: 645 Interesting Engineering
Donate here: http://www.aklectures.com/donate.php Website video link: http://www.aklectures.com/lecture/atomic-radius-ionization-energy-electronegativity-and-electron-affinity Facebook link: https://www.facebook.com/aklectures Website link: http://www.aklectures.com
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Useful for CBSE, ICSE, NCERT & International Students Grade : 10 Subject :Chemistry Lesson :Periodic table of elements Topic: Atomic Size Atomic radii is useful for determining many aspects of chemistry such as various physical and chemical properties. The periodic table greatly assists in determining atomic radius and presents a number of trends. Visit www.oztern.com to find personalized test preparation solutions for Pre Medical - AIPMT, AIIMS, JIPMER, State, Pre Engineering - IIT JEE, JEE MAIN, BITSAT, State and Foundations - Class 6 to 10.
Views: 7510 CBSE
ilmkidunya.com has brought to you Lecture of Sibghat Ullah on "9th Class Chemistry Chapter 3 Periodic Table & Periodicity of Properties. Topic 3.2 Atomic Size and Atomic Radius". For more videos of Sibghat Ullah visit https://www.ilmkidunya.com/study , https://www.instutor.com This lecture is specially recorded for students of 9th class, 9th class from all Punjab Boards and is based on the current curriculum of study for Chemistry book. All these lectures are conducted in Urdu/English medium to facilitate Pakistani students.
Views: 42562 ilmkidunya
Here,I will give you the ever best concept of Atomic size and Atomic radii. In thiss video, I will tell you: 1) Atomic size and atomic radii in the periodic table 2) Atomic radius trends on periodic table | Periodic table | Chemistry | 3) Periodic Trends: Atomic Radius 4) The Periodic Table: Atomic Radius, Ionization Energy, and Electronegativity 5) Periodic Trends in Atomic Size Atomic size is defined interms of atomic radius. Atomic radius means the distance of valence electron from the centre of an atom or nucleus. Atomic size and atomic radii can not be even determined by a powerfull optical microscope. But techniques have been developed to measure the atomic size and atomic radii. Like we find the covalent radius of a molecule then half of the covalent radius is know as atomic radius. When you move from left to right in a periodic table the atomic size and atomic radii decreases. The reason for this is: - The number of protons increase - the number of shells remain the constant Due to which the nuclear attraction on the valence electrons increases. Hence atom becomes condensed, and atomic size and atomic radii decreases. When you move from top to bottom in periodic table the atomic size and atomic radii increases, this is because: - The number of protons are increasing - The number of shells are increasing Due to which the atomic size and atomic radii increases. If we talk about the ionic radii then the cationic radius of ion is always smaller the a neutral atom. This is due to the imbalance of electronic and protonic ratio. In cation, the number of protons are greater then the number of electrons. Therefore nuclear attractions on electrons increase and, atomic size and atomic radii decrease. If we talk about the anionic radii of tis always hen anionic radnumbii is always greater then the neutral atom. this is because the imbalance of the electronic and protonic ratio. In anion, the number of protons is smaller then thenumber of electrons. Therefore nuclear attrctions decrease on electrons and, atomic size and atomic radii decrease. Subscribe my channel at: https://www.youtube.com/channel/UC_ltCdLVMRZ7r3IPzF2Toyg https://www.facebook.com/Najamacademy/ https://www.youtube.com/channel/UC_ltCdLVMRZ7r3IPzF2Toyg
Views: 3548 Najam Academy
Students using nothing but a periodic table to align themselves into a periodic table using their height as the value of their atomic radii. They determine which element they are in relation to other students by their height (atomic radius). The have already graphed this trend with atomic number and have a firm understanding of the trend across periods and groups. They have posted below "acting" like the element they were in the video.
Views: 739 MrGrodskiChemistry
A level Chemistry : A level Chemistry explanation of ionisation and electronegativity
Views: 680 ASFC Chemistry
Periodic Trends | Two Problems | Smallest atomic radii and Ionization energy | Chemistry | Whitwell High School | UTC - University of Tennessee at Chattanooga www.whitwellhigh.com Instructor/Professor: Johnny Cantrell
Views: 2243 Johnny Cantrell
This lecture deals with the first half of the periodic trends including effective nuclear charge and atomic radius. General trends are summarized.
Views: 2651 ChemComplete