CHEM 1A03 Lecture Notes - Lecture 10: Electron Configuration, Sulfur, Ionic Radius

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CHEM 1A03 Full Course Notes

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3. 2. 1 - define the terms first ionisation energy and electronegativity. The energy required to remove one mole of electrons from one mole of atoms in the gaseous state. This shows how tightly the outer-shell electrons are held in an atom. Metals tend to have low ionisation energies because their outer electrons are easily removed. A measure of the attraction an atom has for a for a shared pair of electrons when it is covalently bonded to another atom. Metals have low electronegativities because they lose electrons easily. Non-metals have high electronegativities as they gain electrons to complete their outer shell. Electronegativity tends to increase across a period and up a group. http://ibscrewed4chemistry. blogspot. com/ 3. 2. 2 - describe and explain the trends in atomic radii, ionic radii, first ionisation energies, electronegativities and melting point for the alkali metals and the halogens. Moving down a group, the atomic radii increases.

Related Questions

1)The NaCl2 ionic salt does not exist. Which of the followingstatements best explains why?

A. Because the formation of Na2+ is an unfavorable process due tothe great amount of energy required to remove the 2nd electron fromthe Na atom (the 2nd electron would have to be removed from thecore electrons of the Na atom).
B. Because the Cl- anion is too large for there to be two of themattached to one Na+ ion.
C. Because NaCl2 is actually a polyatomic ion with a -1 charge, andnot an ionic salt. In the presence of another Na+ ion, the Na2Cl2salt would form.
D. Because Cl2 has no charge and therefore would not be attractedelectrostatically to the positively charged Na2+ cation.

2)Select the false statement below.

A. The first ionization energy of an atom is smaller than thesecond ionization energy of the same atom.
B. Phosphorus has a greater first ionization energy than magnesium,and the reason for this is because P has a greater effectivenuclear charge (Zeff) than Mg.
C. The following process is an endothermic process and representsthe first ionization energy of an atom A:A(g) ? A1+(g) + e1-
D. Fluorine has a greater first ionization energy than iodine, andthe reason for this is because fluorine has a greater amount ofshielding of outer electrons by inner electrons than doesiodine.

3)The Group 5A elements N,P,As have lower (less negative) electronaffinities than most of the Group 4A or Group 6A elements becauseN,P,As have half-filled subshells.

True
False

4)A fluorine atom is smaller than a bromine atom, and a potassiumatom is larger than a lithium atom.

True
False

5)A certain main-group element exhibits the following successiveionization energies in kJ/mol:

IE1 = 100; IE2 = 1200; IE3 = 2300; IE4 = 3100; IE5 = 4200

Select the false statement about this element below.

A. This is likely a Group 1A element.
B. This element is typically found uncombined in nature (that is,it is not usually found in compounds, but rather as a freeelement).
C. If this element is given a symbol of "J", it would form an ioniccompound with sulfur as J2S.
D. If this element was in period 2 of the periodic table, it wouldbe lithium.

6)Select the false statement below.

A. Generally speaking, non-metallic elements have greater effectivenuclear charge (Zeff) than metallic elements in the sameperiod.
B. Generally speaking, as you go down a group in the periodictable, there is successively greater shielding of the outer-shellelectrons by the inner-shell electrons.
C. Generally speaking, the heavier alkali metals can be predictedto exhibit greater shielding of the outer-shell electrons by theinner-shell electrons than lighter alkali metals.
D. Generally speaking, as you go across a period in the periodictable, the effective nuclear charge (Zeff) decreases because eachsuccessive element contains more protons in the nucleus than theprevious element and the outer electrons are all in the same shellas you go across a period.

7)Place the following in order of increasing size:

O2-, F1-, Li1+

A. F1- < Li1+ < O2-
B. Li1+ < O2- < F1-
C. Li1+ < F1- < O2-
D. F1- < O2- < Li1+

8)Select the false statement below.

A. The following set of quantum numbers is allowed:
n = 4, l = 2, ml = -2, ms = +1/2
B. The n = 1 shell of any given atom can accomodate up to 2electrons.
C. The n = 4 shell of any given atom can accomodate up to 16electrons.
D. In any given atom, the l = 2 subshell can accomodate up to 5electrons that have negative spins (ms =

redgoldfish403

Question 1 of 15 (worth 2 points)
The NaCl2 ionic salt does not exist. Which of the followingstatements best explains why?

A. Because the formation of Na2+ is an unfavorable process due tothe great amount of energy required to remove the 2nd electron fromthe Na atom (the 2nd electron would have to be removed from thecore electrons of the Na atom).
B. Because Cl2 has no charge and therefore would not be attractedelectrostatically to the positively charged Na2+ cation.
C. Because NaCl2 is actually a polyatomic ion with a -1 charge, andnot an ionic salt. In the presence of another Na+ ion, the Na2Cl2salt would form.
D. Because the Cl- anion is too large for there to be two of themattached to one Na+ ion.
Review
Check to review before finishing (will be flagged in Table ofContents)
Question 2 of 15 (worth 2 points)
Select the false statement below.

A. Fluorine has a greater first ionization energy than iodine, andthe reason for this is because fluorine has a greater amount ofshielding of outer electrons by inner electrons than doesiodine.
B. The following process is an endothermic process and representsthe first ionization energy of an atom A:
A(g) ? A1+(g) + e1-

C. Phosphorus has a greater first ionization energy than magnesium,and the reason for this is because P has a greater effectivenuclear charge (Zeff) than Mg.
D. The first ionization energy of an atom is smaller than thesecond ionization energy of the same atom.
Review
Check to review before finishing (will be flagged in Table ofContents)
Question 3 of 15 (worth 2 points)
The following process represents the first electron affinity of anatom A:

A(g) ? A1+(g) + e1-

True
False
Review
Check to review before finishing (will be flagged in Table ofContents)
Question 4 of 15 (worth 2 points)
Generally speaking, most nonmetal atoms are smaller than most metalatoms.

True
False
Review
Check to review before finishing (will be flagged in Table ofContents)
Question 5 of 15 (worth 2 points)
A certain main-group element exhibits the following successiveionization energies in kJ/mol:

IE1 = 100; IE2 = 1200; IE3 = 2300; IE4 = 3100; IE5 = 4200

Select the false statement about this element below.

A. If this element is given a symbol of "J", it would form an ioniccompound with sulfur as J2S.
B. This element is typically found uncombined in nature (that is,it is not usually found in compounds, but rather as a freeelement).
C. This is likely a Group 1A element.
D. If this element was in period 2 of the periodic table, it wouldbe lithium.
Review
Check to review before finishing (will be flagged in Table ofContents)
Question 6 of 15 (worth 2 points)
Select the false statement below.

A. Generally speaking, as you go down a group in the periodictable, there is successively greater shielding of the outer-shellelectrons by the inner-shell electrons.
B. Generally speaking, non-metallic elements have greater effectivenuclear charge (Zeff) than metallic elements in the sameperiod.
C. Generally speaking, the heavier alkali metals can be predictedto exhibit greater shielding of the outer-shell electrons by theinner-shell electrons than lighter alkali metals.
D. Generally speaking, as you go across a period in the periodictable, the effective nuclear charge (Zeff) decreases because eachsuccessive element contains more protons in the nucleus than theprevious element and the outer electrons are all in the same shellas you go across a period.
Review
Check to review before finishing (will be flagged in Table ofContents)
Question 7 of 15 (worth 2 points)
Place the following in order of increasing size:

O2-, F1-, Li1+

A. F1- < O2- < Li1+
B. F1- < Li1+ < O2-
C. Li1+ < O2- < F1-
D. Li1+ < F1- < O2-
Review
Check to review before finishing (will be flagged in Table ofContents)
Question 8 of 15 (worth 2 points)
Select the false statement below.

A. The n = 4 shell of any given atom can accomodate up to 16electrons.
B. In any given atom, the l = 2 subshell can accomodate up to 5electrons that have negative spins (ms =

CHEM 1A03 Lecture Notes - Lecture 10: Electron Configuration, Sulfur, Ionic Radius

CHEM 1A03 Full Course Notes

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