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CHEM 120 Lecture Notes - Lecture 3: Ionic Radius, Effective Nuclear Charge, Atomic Radius

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violetsheep864
16 Aug 2016
School
Simon Fraser University
Department
Chemistry
Course
CHEM 120
Professor
Tim Storr

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Periodicity (Atomic radii, ionic radii, Trends across the periodic table) Chapter 5
Atomic Radii - the distance between the nucleus and the outer most shell for atoms
Group 1: It increases as the elements become bigger down the group since more
electrons mean more electron shells basically.
Group 7: The same is true for halogens as for alkalis. The elements increase in size down
the group. This is due to more electrons means more full shells which means that the
nucleus of elements attract the outermost electron/s less down the group.
As you move across a period, atomic radius decreases
oAs you go across a period, protons are added to the atom and creates a higher
effective nuclear charge in which the electrons are pulled closer to the nucleus
Ionic Radii - the distance between the nucleus and the outer most shell for ions
Anions - are larger than their atom counterparts
oElectron-electron repulsion forces them to spread further apart
oElectrons outnumber protons, so the protons don’t have enough charge to hold
them in place
Cations - are smaller than their respective atoms
oLess electron electron repulsion, so they can come closer together
oProtons outnumber electrons, so they pull them closer to the nucleus
oIf the electron configuration of the cation is that of a noble gas, then an entire
energy level is lost, in this case, it is much smaller than its atom
https://www.chem.tamu.edu/class/majors/tutorialnotefiles/trends.htm
Ionization Energy
Definition: The energy required to remove a mole the outermost electron from a neutral atom
in its grounds state in kJ/mol
Trends
1.As you move down a group, first ionization energy decreases
a. Electrons are further from the nucleus and easier to remove
b. "Shielding effect" inner electrons at lower E levels block the protons force of
attraction, which makes it easier to remove electrons on the outside
2.As you move across a period, first ionization energy increases
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Document Summary

Periodicity (atomic radii, ionic radii, trends across the periodic table) chapter 5. Atomic radii - the distance between the nucleus and the outer most shell for atoms. Group 1: it increases as the elements become bigger down the group since more electrons mean more electron shells basically. Group 7: the same is true for halogens as for alkalis. The elements increase in size down the group. This is due to more electrons means more full shells which means that the nucleus of elements attract the outermost electron/s less down the group. Ionic radii - the distance between the nucleus and the outer most shell for ions. Anions - are larger than their atom counterparts: electron-electron repulsion forces them to spread further apart o. Electrons outnumber protons, so the protons don"t have enough charge to hold them in place. Cations - are smaller than their respective atoms o.

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Related Questions

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    Please answer these for me im totally confused
    001 10.0 points
    Consider the atoms
    A) nitrogen B) bismuth C) arsenic
    Arrange them in order of increasing first
    ionization energy.
    1. A, C, B
    2. B, A, C
    3. C, B, A
    4. B, C, A
    5. A, B, C
    6. C, A, B


    002 10.0 points
    Which of the following is a measure of the
    tendency of an atom in a molecule to attract
    electrons to itself ?
    1. L nonbonding
    2. polar
    3. electronegativity
    4. ionization


    003 10.0 points
    Which ion has the larger radius?
    1. Unable to determine
    2. Both have same radius.
    3. Sn
    2+
    4. Sn
    4+


    004 10.0 points

    Which of the following statements is true?
    1. Electron affinity is a measure of the
    amount of energy needed to remove an electron from an atom.
    2. As electron affinity increases (becomes
    increasingly negative), electronegativity decreases.
    3. Electronegativity is a measure of the tendency of an atom tolose electrons.
    4. When ionization energy increases, electronegativityincreases.
    5. Ionic radii are always larger than atomic
    radii for the same element.


    005 10.0 points

    Which of the following is a true statement?
    1. There is no relationship between atomic
    size and ionization energy.
    2. Ionization energy increases as electronegativitydecreases.
    3. Electronegativity increases as electron
    affinity decreases (gets more positive).
    4. None of these
    5. Ionization energy increases as atomic size
    decreases.


    006 10.0 points
    Which of the following correctly rationalizes
    the increase in atomic radii down and to the
    left on the periodic table, based on what we
    discussed in class?
    1. None of these. Atomic radii increase up
    and to the right.
    2. Because the elements are easier to ionize, they have a largerelectronegativity, and
    therefore their electron affinity is not suffi-
    cient to reduce atomic radii.penwell (blp865) – HW 12 PeriodicTrends – thompson – (991918292) 2
    3. Larger elements have an increasing proportion of d and forbitals, which are intrinsically larger than all of the s and porbitals.
    4. As you move to the left across a period,
    decreasing ENC means the outer electrons
    are less tightly held and can move further
    from the nucleus. As you move down a group,
    the electrons occupy orbitals that are further
    from the nucleus.
    5. The elements are simply larger due to
    more protons and neutrons.
    6. The periodic table was set up to group
    atoms by size to facilitate comparisons.


    007 10.0 points
    In a series of species with the same total set
    of electrons present, one observes that
    1. the radii would increase as the atomic
    number increases.
    2. the radii would decrease as the atomic
    number increases.
    3. the radii would decrease as the number of
    electrons increases.
    4. all have the same radius.
    5. the radii would increase as the number of
    electrons increases.


    008 10.0 points
    The ions Na
    +
    , F
    −
    , and O
    2−
    each have ten
    electrons. What would be the order of the
    sizes of these three ions?
    1. Na
    +
    is smaller than O
    2−
    which is smaller
    than F
    −
    .
    2. O
    2−
    is smaller than Na
    +
    which is smaller
    than F
    −
    .
    3. F
    −
    is smaller than O
    2−
    which is smaller
    than Na
    +
    .
    4. F
    −
    is smaller than Na
    +
    which is smaller
    than O
    2−
    .
    5. Na
    +
    is smaller than F
    −
    which is smaller
    than O
    2−
    .
    009 10.0 points
    Which of the following atoms has the largest
    radius?
    1. K
    2. Mg
    3. Li
    4. Br
    5. Si
    010 10.0 points
    Why is it harder to remove an electron from
    fluorine than from carbon, or, to put it another way, why are thevalence electrons of
    fluorine more strongly bound than those of
    carbon?
    1. The valence electrons of both fluorine and
    carbon are found at about the same distance
    from their respective nuclei but the greater
    positive charge of the fluorine nucleus attracts
    its valence electrons more strongly.
    2. Fluorine has more valence elctrons than
    does carbon.
    3. Carbon has a lower atomic mass than
    does fluorine.
    4. Fluorine has a nearly filled octet, which
    is always more stable than a partially filled
    octet.
    5. The statement is false; it takes very nearly
    the same energy to remove an electron from
    (ionize) both elements.
    011 10.0 points
    In general, ionization energy tends to increasepenwell (blp865) –HW 12 Periodic Trends – thompson – (991918292) 3
    in the periodic table
    1. from bottom to top and from right to
    left.
    2. in no regular trend.
    3. from bottom to top and from left to
    right.
    4. from top to bottom and from right to
    left.
    5. from top to bottom and from left to
    right.
    012 10.0 points
    Consider the most stable ions which are
    formed by the elements Cs, Ba, Te and I.
    Which element will form the ion with the
    largest radius? (Hint: the ions will be isoelectronic.)
    1. Ba
    2. Te
    3. Cs
    4. I
    013 10.0 points
    Which of the following has the largest radius?
    1. S
    2−
    2. K
    +
    3. Cl
    4. Cl
    −
    5. S
    014 10.0 points
    What is the order of decreasing ionization
    energy?
    1. tellurium, selenium, oxygen
    2. oxygen, selenium, tellurium
    3. selenium, oxygen, tellurium
    4. selenium, tellurium, oxygen
    5. oxygen, tellurium, selenium
    6. tellurium, oxygen, selenium
    015 10.0 points
    Which atom is smaller?
    1. Unable to determine
    2. bromine
    3. iodine
    4. They have the same size.
    016 10.0 points
    Rank the following species from smallest to
    largest atomic radius: K, Mg, Rb, Ca.
    1. Rb < K < Ca < Mg
    2. Mg < Ca < K < Rb
    3. Mg < Ca < Rb < K
    4. Mg < Rb < K < Ca
    5. Mg < K < Ca < Rb
    017 10.0 points
    Francium (atomic number 87) would be expected to have a (large,small) first ionization
    potential and a (large, small) electronegativity.
    1. large; large
    2. small; small
    3. large; small
    4. small; largepenwell (blp865) – HW 12 Periodic Trends – thompson– (991918292) 4
    018 10.0 points
    Consider the following ground-state electronic
    configurations. Which atom has both the
    highest first ionization energy and the highest
    electron affinity?
    1. [Ne] 3s
    2
    3p
    4
    2. [Ne] 3s
    2
    3p
    5
    3. [Ne] 3s
    2
    3p
    1
    4. [Ne] 3s
    2
    3p
    3
    019 10.0 points
    The energy needed to remove electrons from
    an atom is called
    1. bonding energy.
    2. ionization energy.
    3. valence energy.
    4. network energy.
    020 10.0 points
    Rank the following atoms and ions
    Li
    +
    , Be
    2+
    , He, H
    −
    , B
    3+
    in order of decreasing size.
    1. B
    3+
    , Be
    2+
    , Li
    +
    , He, H
    −
    2. B
    3+
    , Be
    2+
    , He, Li
    +
    , H
    −
    3. H
    −
    , Li
    +
    , He, Be
    2+
    , B
    3+
    4. He, H
    −
    , Li
    +
    , Be
    2+
    , B
    3+
    5. H
    −
    , He, Li
    +
    , Be
    2+
    , B
    3+
    021 10.0 points
    Rank the following in terms of decreasing
    ionic radii.
    1. F
    −
    , O
    2−
    , N
    3−
    , Na
    +
    , Mg
    2+
    2. Na
    +
    , Mg
    2+
    , O
    2−
    , N
    3−
    , F
    −
    3. N
    3−
    , O
    2−
    , F
    −
    , Na
    +
    , Mg
    2+
    4. Mg
    2+
    , Na
    +
    , F
    −
    , O
    2−
    , N
    3−
    5. Na
    +
    , Mg
    2+
    , N
    3−
    , O
    2−
    , F
    −
    022 10.0 points
    What is the order of decreasing atomic radius?
    1. chromium, titanium, cobalt
    2. titanium, cobalt, chromium
    3. cobalt, titanium, chromium
    4. titanium, chromium, cobalt
    5. cobalt, chromium, titanium
    6. chromium, cobalt, titanium
    023 10.0 points
    Atoms with loosely held valence electrons
    have
    1. high ionization energy and high electron
    affinity.
    2. low ionization energy and low electron
    affinity.
    3. low ionization energy and high electron
    affinity.
    4. high ionization energy and low electron
    affinity.