Unit 5 review

Which electrons were gained or lost to complete the outer octet and produce the following ions? P³⁻

3p

Predict the oxidation number of the following elements. B

3⁺

Predict the oxidation numbers for the following elements. Al

3⁺

Predict the oxidation numbers of the following elements Bi

3⁺

Predict the oxidation numbers of the following elements Pu

3⁺, 4⁺,6⁺

Predict the oxidation number of the following elements. P

3⁻

Predict the oxidation numbers for the following elements. N

3⁻

In each of the following pairs of particles, pick the one that is smaller. Fe, Fe³⁺

Fe³⁺

Predict the oxidation number of the following elements. Ar

0

Which electrons were gained or lost to complete the outer octet and produce the following ions? Sc³⁺

1 3d, 2 4s

Which electrons were gained or lost to complete the outer octet and produce the following ions? Br⁻

1 4p

For each element listed below, determine the charge of the ion most likely to be formed and the identity of the noble gas whose electron configuration is thus achieved Li

1+ , He

For each element listed below, determine the charge of the ion most likely to be formed and the identity of the noble gas whose electron configuration is thus achieved Br

1-, Kr

For each element listed below, determine the charge of the ion most likely to be formed and the identity of the noble gas whose electron configuration is thus achieved F

1-, Ne

How do the values of successive ionization energies compare?

1st < 2nd < 3rd

Distinguish among the first, second, and third ionization energies of an atom.

1st IE is the energy required to remove the 1st electron, 2nd IE is the energy required to remove the second electron, and 3rd IE is the energy required to remove the 3rd electron.

Predict the oxidation number of the following elements. K

1⁺

Predict the oxidation number of the following elements. LI

1⁺

Predict the oxidation numbers for the following elements. Na

1⁺

Predict the oxidation numbers of the following elements Rb

1⁺

Predict the oxidation number of the following elements. F

1⁻

Which electrons were gained or lost to complete the outer octet and produce the following ions? Ca²⁺

2 4s

Which electrons were gained or lost to complete the outer octet and produce the following ions? Ga³⁺

2 4s, 1 4p

Which electrons were gained or lost to complete the outer octet and produce the following ions? Sn⁴⁺

2 5s, 2 5p

For each element listed below, determine the charge of the ion most likely to be formed and the identity of the noble gas whose electron configuration is thus achieved Mg

2+, Ne

For each element listed below, determine the charge of the ion most likely to be formed and the identity of the noble gas whose electron configuration is thus achieved Ba

2+, Xe

For each element listed below, determine the charge of the ion most likely to be formed and the identity of the noble gas whose electron configuration is thus achieved S

2-, Ar

For each element listed below, determine the charge of the ion most likely to be formed and the identity of the noble gas whose electron configuration is thus achieved O

2-, Ne

Which electrons were gained or lost to complete the outer octet and produce the following ions? O²⁻

2p

Predict the oxidation number of the following elements. Be

2⁺

Predict the oxidation numbers for the following elements. Mg

2⁺

Predict the oxidation numbers for the following elements. Zn

2⁺

Predict the oxidation numbers of the following elements Ba

2⁺

Predict the oxidation numbers of the following elements Co

2⁺ or 3⁺

Predict the oxidation numbers of the following elements V

2⁺, 3⁺, 4⁺, 5⁺

Predict the oxidation numbers for the following elements. Mn

2⁺, 7⁺

Predict the oxidation number of the following elements. O

2⁻

Predict the oxidation numbers for the following elements. Cl

2⁻

Predict the oxidation numbers for the following elements. S

2⁻, 4⁺, 6⁺

For each element listed below, determine the charge of the ion most likely to be formed and the identity of the noble gas whose electron configuration is thus achieved B

3+, He

For each element listed below, determine the charge of the ion most likely to be formed and the identity of the noble gas whose electron configuration is thus achieved Al

3+, Ne

For each element listed below, determine the charge of the ion most likely to be formed and the identity of the noble gas whose electron configuration is thus achieved P

3-, Ar

Which electrons were gained or lost to complete the outer octet and produce the following ions? K⁺

4s

Predict the oxidation number of the following elements. C

4⁺ or 4⁻

Which atom in each of the following pairs would have the lower first ionization energy? Al, N

Al

From each of the following pairs, use the periodic table to select the atom that is larger in radius. Ac, U

Ac

From each of the following pairs of particles, select the particle that is larger in radius. Ag, Ag⁺

Ag

From each of the following pairs, use the periodic table to select the atom that is larger in radius. B, Al

Al

In each of the following pairs of atoms, pick the one that is larger. Al, B

Al

In each of the following pairs of atoms, pick the one that is larger. Ne, Ar

Ar

In each of the following pairs of particles, pick the one that is smaller. As³⁻, As

As

From each of the following pairs of particles, select the particle that is larger in radius. As³⁻, P³⁻

As³⁻

From each of the following pairs, use the periodic table to select the atom that is larger in radius. Au, Ba

Ba

In each of the following pairs of atoms, pick the one that is larger. Br, C

Br

In each of the following pairs of particles, pick the one that is smaller. Br⁻, Se²⁻

Br⁻

From each of the following pairs of particles, select the particle that is larger in radius. Ca, Ca²⁺

Ca

Which atom in each of the following pairs would have the lower first ionization energy? Mg, Ca

Ca

Which among the following does not have a noble gas configuration: Na⁺, Rb⁺, O²⁻, Br⁻, Ca⁺, Al³⁺, S²⁻?

Ca+

The two ions K+ and Ca2+ each have 18 electrons surrounding the nucleus. Which would you expect to have the smaller radius? Why?

Ca2+ because it has 20 protons to pull the nucleus in where K+ only has 19 protons.

From each of the following pairs of particles, select the particle that is larger in radius. F⁻, Cl⁻

Cl⁻

From each of the following pairs of particles, select the particle that is larger in radius. C, C⁴⁻

C⁴⁻

Why does this occur?

Each successive electron must be removed from a particle with an increasingly larger charge.

Which atom in each of the following pairs would have the lower first ionization energy? Ne, F

F

Without looking at the electronegativity table, arrange the elements listed in order of decreasing electronegativities: C, O, Li, Na, Rb, Ne, and F.

F > O > C > Li > Na > Rb > Be

Which atom in each of the following pairs would have the lower first ionization energy? C, Ge

Ge

From each of the following pairs, use the periodic table to select the atom that is larger in radius. Cl, I

I

Which atom in each of the following pairs would have the lower first ionization energy? Br, I

I

In each of the following pairs of atoms, pick the one that is larger. K, Ca

K

Which of the following ions is least likely to form: I⁻, Sr²⁺, Al³⁺, Cl⁻, O²⁻, K²⁺?

K2+

Which would you expect to have the highest second ionization energy? Why? refer to Without looking at the ionization energy table, arrange the elements listed in order of decreasing first ionization energies: Li, O, C, K, Ne, and F.)

Li - both Li and K only have 1 valence electron but Li+ is smaller than K+

From each of the following pairs, use the periodic table to select the atom that is larger in radius. Mg, Be

Mg

From each of the following pairs of particles, select the particle that is larger in radius. Mg²⁺, Be²⁺

Mg²⁺

In each of the following pairs of particles, pick the one that is smaller. Mo³⁺, Mo

Mo³⁺

In each of the following pairs of atoms, pick the one that is larger. F, N

N

Which atom in each of the following pairs would have the lower first ionization energy? N, O

N

In each of the following pairs of atoms, pick the one that is larger. Mg, Na

Na

Without looking at the ionization energy table, arrange the elements listed in order of decreasing first ionization energies: Li, O, C, K, Ne, and F.

Ne > F > O > C > Li > K

From each of the following pairs, use the periodic table to select the atom that is larger in radius. S, P

P

From each of the following pairs of particles, select the particle that is larger in radius. Pb⁺⁴, Pb

Pb

From each of the following pairs, use the periodic table to select the atom that is larger in radius. Na, Rb

Rb

In each of the following pairs of particles, pick the one that is smaller. S²⁻, S

S

Which atom in each of the following pairs would have the lower first ionization energy? F, S

S

Which atom in each of the following pairs would have the lower first ionization energy? I, Sb

Sb

Which atom in each of the following pairs would have the lower first ionization energy? Te, Sn

Sn

From each of the following pairs, use the periodic table to select the atom that is larger in radius. Sn, Sr

Sr

From each of the following pairs of particles, select the particle that is larger in radius. Te²⁻, Te

Te²⁻

In each of the following pairs of particles, pick the one that is smaller. Ac³⁺, U³⁺

U³⁺

As the distance between the nucleus and the outer electrons of an atom increases, will the ionization energy increase or decrease?

decrease

Does the radii of atoms within a period increase or decrease as the atomic number increases?

decrease

In a group, will the ionization energy tend to increase or decrease with increasing atomic number?

decrease

As the shielding effect increases, will the ionization energy increase or decrease?

decreases

In a period, will the ionization energy tend to increase or decrease with increasing atomic number?

increase

Within a group, does the radii of atoms increase or decrease as the atomic number increases?

increase

As the positive charge on an ion increases, will the ionization energy increase or decrease?

increases

Carbon has a first ionization energy of 1086.5 kJ/mol. Predict whether the first ionization energies of the following elements will be more or less than that of carbon? lithium

less

Carbon has a first ionization energy of 1086.5 kJ/mol. Predict whether the first ionization energies of the following elements will be more or less than that of carbon? silicon

less

Do metals or nonmetals generally have lower ionization energies?

metals

Carbon has a first ionization energy of 1086.5 kJ/mol. Predict whether the first ionization energies of the following elements will be more or less than that of carbon? fluorine

more

Carbon has a first ionization energy of 1086.5 kJ/mol. Predict whether the first ionization energies of the following elements will be more or less than that of carbon? helium

more