Chem Ch 7-8

Front 1

In 1913, the English physicist Henry Moseley developed the concept of atomic numbers. He correctly identified the atomic number with which of the following?

The atomic weight of an atom.

The number of protons and neutrons in the nucleus of an atom.

The number of protons in the nucleus of the atom and the number of electrons in the atom.

The number of neutrons in the nucleus of the atom.

Back 1

The number of protons in the nucleus of the atom and the number of electrons in the atom.

Front 2

Which of the following occurs upon moving from left to right across a period (row) of elements on the periodic table?

The number of core electrons changes.

The principal quantum number decreases.

The effective nuclear charge increases.

The principal quantum number increases.

Back 2

The effective nuclear charge increases.

Front 3

Which list correctly gives atoms in order of increasing size?

Cl < P < Xe < Br

P < Cl < Br < Xe

Xe < Br < P < Cl

Cl < P < Br < Xe

Back 3

Cl < P < Br < Xe

Front 4

Which of the following shows a correct relationship between first ionization energies of the given atoms?

Xe > Ne

Ne > F

Li > Be

Ga > Ge

Back 4

Ne > F

Front 5

Electron affinity is ____ when energy is absorbed, and it is ______ when energy is released.

Back 5

positive; negative

Front 6

Positive or Negative electron affinity?

Ar 1s22s22p63s23p6

Ar(g) + 1e- ---> Ar-(g)

Back 6

Positive

Front 7

Positive or Negative electron affinity?

Br 1s22s22p63s23p64s23d104p5

Br(g) + 1e- ---> Br-(g)

Back 7

Negative

Front 8

Positive or Negative electron affinity?

Na 1s22s22p63s1

Na(g) + 1e- ---> Na-(g)

Back 8

Negative

Front 9

Positive or Negative electron affinity?

Mg 1s22s22p63s2

Mg(g) + 1e- ----> Mg-(g)

Back 9

Positive

Front 10

Positive or Negative electron affinity?

Cl− 1s22s22p63s23p6

Cl-(g) + 1e- ---> Cl^2-(g)

Back 10

Positive

Front 11

Consider the addition of an electron to the following atoms from the fifth period. Rank the atoms in order from the most negative to the least negative electron affinity values based on their electron configurations.

I [Kr]4d105s25p5

Sn [Kr]4d105s25p2

Xe [Kr]4d105s25p6

Back 11

I, Sn, Xe

Front 12

Which of the following correctly describes the measurement of an atom's electron affinity?

It is a positive value.

It is a measure of the ease with which an atom loses an electron.

It is a measurement of the energy change associated with forming a positively charged ion from a neutral atom.

It measures the ease with which an atom gains an electron.

Back 12

It measures the ease with which an atom gains an electron.

Front 13

Which of the following correctly lists nonmetals that exist under ordinary conditions as diatomic molecules?

Cl, N, P, O.

Cl, Br, F, O.

I, Kr, Br, H.

H, N, Cl, Ge.

Back 13

Cl, Br, F, O

Front 14

Metalloids have properties intermediate between those of metals and nonmetals. An example of a metalloid is _____.

P.

Al.

I.

Sb.

Back 14

Sb

Front 15

Which halogen is a liquid at room temperature?

bromine. fluorine. iodine. mercury.

Back 15

bromine

Front 16

Which of the following is an allotrope of O2?

H2O2. SO2. H2O. O3.

Back 16

O3

Front 17

Looking at the periodic table on the inside front cover in the textbook, can you find an example other than Ar and K where the order of the elements would be different if the elements were arranged in order of increasing atomic weight?Check all that apply.

Be/B

Cu/Zn

Cf/Es

Co/Ni

Tc/Ru

Te/I

Back 17

Co/Ni; Te/I

Front 18

Which would you expect to experience a greater effective nuclear charge?

a 2p electron of a Ne atom

a 3s electron of a Na atom

Back 18

a 2p electron of a Ne atom

Front 19

Rank the following elements in order of decreasing atomic radius.

Br, I, Cl, F

Back 19

I, Br, Cl, F

Front 20

Rank the following elements in order of decreasing atomic radius.

Mg, Si, Al, Na

Back 20

Na Mg Al Si

Front 21

The shielding of electrons gives rise to an effective nuclear charge, Zeff, which explains why boron is larger than oxygen. Estimate the approximate Zeff felt by a valence electron of boron and oxygen, respectively?

+5 and +8.

+3 and +6.

+5 and +6.

+3 and +8.

+1 and +4

Back 21

+3 and +6

Front 22

In Section 7.2 in the textbook we said that Zeff generally increases when you move down a column of the periodic table, whereas in Chapter 6 we saw that the "size" of an orbital increases as the principal quantum number n increases.

With respect to atomic radii, do these trends work together or against each other?

Back 22

These trends work against each other.

Front 23

Which effect is larger?

the orbital size effect.

the Zeff effect.

Back 23

the orbital size effect

Front 24

How do cations of the same charge change in radius as you move down a column in the periodic table?

They get larger, just like the atoms do.

They get larger, inversely to the atoms do.

They get smaller, just like the atoms do.

They get smaller, inversely to the atoms do.

Back 24

They get larger, just like the atoms do.

Front 25

Arrange the elements in decreasing order of first ionization energy.

Ge, Cs, In, Se

Back 25

Se, Ge, In, Cs

Front 26

Arrange the elements in order of decreasing first ionization energy.

Element: Radius(pm)

X:111Y:191Z:254

Back 26

element X, element Y, element Z

Front 27

Which would you expect to be greater?

I2 for a carbon atom

I1 for a boron atom

Back 27

I2 for a carbon atom

Front 28

Why it is easier to remove a 2p electron from an oxygen atom than from a nitrogen atom.

It is easier to remove a 2p electron from an oxygen atom because oxygen is more electronegative than nitrogen.

There is more electron–electron repulsion in the case of oxygen because two electrons have to occupy the same orbital.

In the case of oxygen there are more electrons in the atom so they have to move in a higher radii orbite and can easier separate.

In oxygen atom the nucleus is much smaler so attraction between it and electrons is lower.

Back 28

There is more electron–electron repulsion in the case of oxygen because two electrons have to occupy the same orbital.

Front 29

Which of the two processes shown in the following equations requires shorter-wavelength radiation?

Na(g)→Na+(g)+e−

Na+(g)→Na2+(g)+e−

Back 29

Na+(g)→Na2+(g)+e−

Front 30

Do Cr3+ and V2+ have the same or different electron configurations?

Back 30

the same

Front 31

What is the relationship between the value for the first ionization energy of a Cl−(g) ion and the electron affinity of Cl(g)?

They coincide completely.

The numbers are the same; the signs are opposite.

The numbers are different; the signs are the same.

There are no relationship between the values.

Back 31

The numbers are the same; the signs are opposite

Front 32

A compound ACl3 (A is an element) has a melting point of -112 ∘C.

Would you expect the compound to be molecular or ionic?

Back 32

molecular

Front 33

A compound ACl3 (A is an element) has a melting point of -112 ∘C.

If you were told that A is either scandium or phosphorus, which do you think is the more likely choice?

ScCl3.

PCl3.

Back 33

PCl3

Front 34

Antimony forms binary compounds with Cl and with Mg.

Will it be in the same oxidation state in these two compounds?

Back 34

No, it will be different oxidation state.

Front 35

If we had potassium vapor lamps, what color would they be?

red. blue. lilac. green.

Back 35

lilac

Front 36

Cesium tends to be the most reactive of the stable alkali metals (francium, Fr, is radioactive and has not been extensively studied).

What atomic property of Cs is most responsible for its high reactivity?

small atomic size.

high melting point.

low ionization energy.

high Zeff.

Back 36

low ionization energy

Front 37

How many dots should be shown in the Lewis symbol for phosphorus?

One. Five. Six. Seven.

Back 37

Five

Front 38

Consider the lattice energy of any ionic compound. What combination of ions and charges will produce the largest (in magnitude) lattice energies?

small ions and small charges.

large ions and large charges.

small ions and large charges.

large ions and small charges.

Back 38

small ions and large charges

Front 39

Rank the following compounds from largest to smallest according to their expected magnitude in lattice energy.

MgS, KBr, CsI, BeO, KI

Back 39

BeO, MgS, KBr, KI, CsI

Front 40

Which of the following shows the correct order of increasing lattice energy for the given compounds?

K2O < Na2O < Li2O.

Na2O < K2O < Li2O.

Li2O < Na2O < K2O.

Na2O < Li2O < K2O.

Back 40

K2O < Na2O < Li2O

Front 41

Which of the following is isoelectronic with P3−?

O2−

Na+

K+

N3−

Back 41

K+

Front 42

In many molecules, atoms attain complete octet by sharing more than one pair of electrons. Which of the following correctly describes a triple covalent bond?

It results in a shorter distance between the bonded atoms than does a single bond.

It is formed when two chlorine atoms form covalent bonds.

It results in a longer distance between the bonded atoms than does a single bond.

It corresponds to the sharing of two pairs of electrons.

Back 42

It results in a shorter distance between the bonded atoms than does a single bond.

Front 43

The C−O bond length in carbon monoxide, CO, is 1.13Å, whereas the C−O bond length in CO2 is 1.24Å.

Without drawing a Lewis structure, do you think that CO contains a single, double, or triple bond?

Back 43

triple

Front 44

Ionic, Polar Covalent, or Nonpolar Covalent?

(Be = 1.5, F = 4.0)

Be and F

Back 44

Ionic (1.5 - 4.0 = 2.5)

Front 45

Ionic, Polar Covalent, or Nonpolar Covalent?

(S = 2.5, I = 2.5)

S and I

Back 45

Nonpolar Covalent (2.5 - 2.5 = 0)

Front 46

Ionic, Polar Covalent, or Nonpolar Covalent?

(S = 2.5, O = 3.5)

S and O

Back 46

Polar Covalent (2.5 - 3.5 = 1.0)

Front 47

Ionic, Polar Covalent, or Nonpolar Covalent?

(Sc = 1.3, O = 3.0)

Sc and O

Back 47

Ionic (1.3 - 3.0 = 1.7)

Front 48

Ionic, Polar Covalent, or Nonpolar Covalent?

(Be = 1.5, Cl = 3.0)

Be and Cl

Back 48

Polar Covalent (1.5 - 3.0 = 1.5)

Front 49

Ionic, Polar Covalent, or Nonpolar Covalent?

(H = 2.1, P = 2.1)

H and P

Back 49

Nonpolar Covalent (2.1 - 2.1 = 0)

Front 50

Ionic, Polar Covalent, or Nonpolar Covalent?

(H = 2.1, Br = 2.8)

H and Br

Back 50

Polar Covalent (2.1 - 2.8 = 0.7)

Front 51

Nonpolar Covalent =

Back 51

0

Front 52

Polar Covalent =

Back 52

less than 2 but greater than 0

Front 53

Ionic =

Back 53

An ionic bond results when the sharing is so unequal that fully charged ions form.

Front 54

Which of the following compounds has the highest boiling point?

(Metals have low electronegativity compared to nonmetals. So in general, we can predict that any metal–nonmetal combination will be ionic and any nonmetal–nonmetal combination will be covalent. If electronegativity values aren't given, you should assume that a covalent bond is polar unless it is between two atoms of the same element.)

F2.

NaF.

HF.

ClF.

Back 54

NaF

Front 55

Consider the covalent bond each of the following elements forms with hydrogen: chlorine, phosphorus, sulfur, and silicon.

Which will form the most polar bond with hydrogen?

Cl.

Si.

P.

S.

Back 55

Cl

Front 56

For the group 6A elements, what is the trend in electronegativity with increasing atomic number?

The electronegativity increases with increasing atomic number.

The electronegativity decreases with increasing atomic number.

The electronegativity stays the same with increasing atomic number.

Back 56

The electronegativity decreases with increasing atomic number.

Front 57

The bond between carbon and hydrogen is one of the most important types of bonds in chemistry. The length of a H−C bond is approximately 1.1Å.

Based on this distance and differences in electronegativity, do you expect the dipole moment of an individual H−C bond to be larger or smaller than that of the H−I bond?

Back 57

smaller

Front 58

Chlorine monofluoride, ClF, and iodine monofluoride, IF, are interhalogen compounds compounds that contain bonds between different halogen elements.

Which of these molecules has the larger dipole moment?

ClF. IF.

Back 58

IF

Front 59

In the correct Lewis structure for the nitrate ion, NO3 –­, nitrogen has how many covalent bonds?

three. four. six. five.

Back 59

four

Front 60

Benzene, an aromatic organic compound, is often represented as a hexagon with a circle in it to emphasize which of the following?

That the hydrogen atoms need not be shown.

That there are two equivalent Lewis structures that can be drawn.

That only one Lewis structure can be drawn that satisfies the octet. See section 8.06.

That no resonance structures can be drawn for benzene.

Back 60

That there are two equivalent Lewis structures that can be drawn.

Front 61

Which of the following atoms could have an expanded octet when it is the central atom in a covalent compound?

F. O. Cl. B.

Back 61

Cl

Front 62

What is the bond order of F2?

Back 62

1

Front 63

What is the bond order of SO?

Back 63

2

Front 64

What is the bond order of N2?

Back 64

3

Front 65

Rank the following molecules or ions in order of decreasing bond energy:

fluorine: F2, sulfur monoxide: SO, nitrogen: N2

Back 65

Nitrogen, Sulfur Monoxide, Fluorine

Front 66

Rank the following molecules or ions in order of decreasing bond length:

fluorine: F2, sulfur monoxide: SO, nitrogen: N2

Back 66

Fluorine, Sulfur Monoxide, Nitrogen

Front 67

1. Cations have a ______ radius than their neutral atoms and anions have a ______ radius. Because Na and Cl are in the same row of the periodic table, we would expect _____ to have a smaller radius than ____, so we would guess that the larger green spheres represent ___.

Back 67

smaller; larger; Na+; Cl−; Cl−

Front 68

Describe the electron transfers that occur in the formation of calcium fluoride from elemental calcium and elemental fluorine.

Each Ca atom transfers two electrons to each fluorine atom.

Each Ca atom transfers two electrons to each of two fluorine atoms.

Each Ca atom transfers one electron to each of two fluorine atoms.

Each Ca atom transfers one electron to each fluorine atom.

Back 68

Each Ca atom transfers one electron to each of two fluorine atoms.

Front 69

_______ measures the __ released when an isolated atom ___ and electron o form a __ ion. _____ measures the ___ of the atom to hold onto its own electrons and attract electrons from other atoms in compounds.

Back 69

Electron affinity, energy, gains, 1-, the electronegativity, ability

Front 70

If you were to perform the reaction KBr (s)→K+ (g)+ Br−(g), would energy be absorbed or released? (KBr = 671)

The value for the lattice energy is ____, which means the reaction is ____ and, therefore, energy is ____.

Back 70

positive, endothermic, absorbed

Front 71

Which element forms a 3+ ion that has the electron configuration [Kr]4d6 ?

Back 71

Rh

Front 72

ou have a yellow solid that melts at 41∘C and boils at 131∘C and a green solid that melts at 2320∘C.

If you are told that one of them is Cr2O3 and the other is OsO4, which one do you expect to be the yellow solid?

Cr2O3.

OsO4.

Back 72

OsO4

Front 73

If the charged particles are moved closer together, does μ increase, decrease, or stay the same?

μ will increase.

μ will stay the same.

μ will decrease.

Back 73

μ will decrease

Front 74

In the same sense that we describe the O−O bonds in O3 as "one-and-a-half" bonds, how would you describe the N−O bonds in NO3−?

as "one-and-a-fourth" bonds.

as "one-and-a-half" bonds.

as "one-and-a-third" bond.

as a single bond.

Back 74

as "one-and-a-third" bonds

Front 75

Based on bond enthalpies, which do you expect to be more reactive?

hydrogen peroxide, H2O2.

oxygen, O2.

Back 75

hydrogen peroxide, H2O2