Chemistry Chapter 8 Learnsmart Questions

Front 1

The original periodic table...

Back 1

... predicted the properties of elements that were not discovered until later, had elements arranged by atomic mass, had 65 elements, and was developed by Dmitri Mendeleev.

Front 2

The electron configuration of an element describes _____.

Back 2

the distribution of electrons in the orbitals of its atoms.

Front 3

core electrons...

Back 3

are electrons in the previous noble gas and any filled d or f sublevels

Front 4

outer electrons...

Back 4

are electrons in the highest energy level that contains electrons

Front 5

valence electrons...

Back 5

electrons involved in bonding.

Front 6

What accounts for the observation that Li, Na, K and Cs have similar chemical properties...

Back 6

They have the same outer electron configuration.

Front 7

The ground-state electron configuration obeys...

Back 7

both the aufbau principle and Hund's rule.

Front 8

For many-electron systems each principal energy level is split into _____ of differing energies. The energy of an orbital in such a system is affected by the _____ charge, by repulsions between _____, and by orbital shape.

Back 8

sublevels

nuclear

electrons

Front 9

Based on periodic trends, which elements (C, Sb, Ba & F)...

... most readily forms a cation.

... forms acidic oxides.

... most readily gains electrons.

... is the most metallic metalloid in its group.

Back 9

C... forms acidic oxides.

Sb... is the most metallic in its group.

Ba... most readily forms a cation.

F... most readily gains electrons.

Front 10

Ranking of energy levels from lowest to highest.

Back 10

S < P < D < F

Front 11

The first three quantum numbers describe the _____ a particular electron is in whereas the fourth quantum number describes the _____ of an electron.

Back 11

orbital

spin

Front 12

Ground-state electron configurations...

Back 12

... are the basis for the recurring pattern of chemical behavior and they have the lowest-energy distribution of the electrons.

Front 13

The spin quantum number...

Back 13

is a property of the electron itself and will have a value of +1/2 or -1/2.

Front 14

Arrange the following elements in order of increasing atomic size, starting with the smallest atom at the top of the list:

I, Se, Br, S

Back 14

S

Br

Se

I

Front 15

When forming an ion, main-group s-block metals...

Back 15

lose all electrons from the ns sublevel.

Front 16

When forming an ion, main-group p-block metals...

Back 16

lose first the np electrons, then the ns electrons.

Front 17

When forming an ion, main-group nonmetals...

Back 17

gain electrons to fill the np sublevel.

Front 18

When forming an ion, transition metals...

Back 18

lose ns electrons before losing (n-1)d electrons.

Front 19

Electron-electron repulsions result in each electron _____.

Back 19

shielding the other electrons from the nucleus.

Front 20

Metal oxides are _____ and basic, whereas nonmetal oxides are _____ and acidic.

Back 20

ionic

covalent

Front 21

An atom of Sn (Z=50) has _____ inner (core) electrons, _____ outer electrons and _____ valence electrons.

Back 21

46 inner electrons

4 outer electrons

4 valence electrons

Front 22

Electron configuration can be designated using a shorthand notation of the general form nl# (e.g., 1s²). What do n, l, and # mean?

Back 22

n = principal energy level or shell of the relevant electrons

l = sublevel of the relevant electrons

# = number of electrons in the given sublevel.

Front 23

Arrange the following elements in order of increasing ionization energies (IE) starting with the element that has the lowest IE at the top of the list.

K, Rb, Br, Ca

Back 23

Rb

K

Ca

Br

Front 24

Why does atomic size generally increase down a group on the periodic table?

Back 24

The outer electrons are increasingly further away from the nucleus and shielded more effectively by additional shells of inner electrons.

Front 25

Elements that are in the same _____ of the periodic table will have the same _____ electron configuration and will have very similar chemical _____.

Back 25

group

outer

behavior

Front 26

Which of the following elements exhibit an irregular filling pattern of the orbitals? Select all that apply.

Cr, Cd, Cu, Sc, W

Back 26

Cr & Cu

Front 27

Which of the following monatomic ions have the electron configuration 1s² 2s² 2p⁶?

F⁻, S²⁻, O²⁻, Li⁺, Na⁺

Back 27

F⁻

O²⁻

Na⁺

Front 28

List the following elements in order of decreasing atomic size, starting with the largest at the top: He, B, Li, N

Back 28

Li

B

N

He

Front 29

IE decreases _____

IE increases _____

Back 29

down a group

from left to right across a period

Front 30

For a many-electron atom, which of the following sublevels has the highest energy?

3s, 4s, 3p, 3d

Back 30

3d

Front 31

Which of the following elements is expected to have the highest first ionization energy, based on periodic trends? Ca, Ne, P, Cl

Back 31

Ne

Ionization energy is closely related to effective nuclear charge. Ne is in Period 2 and its outermost electrons are therefore in the second principal energy level or shell. It is harder to remove one of these electrons than to remove an electron from the third principal energy level.

Front 32

Hund's rule states that when a sublevel contains several orbitals of equal energy, _____ electron(s) must be placed in each orbital before electrons are _____.

Back 32

one

paired

Front 33

Which of the following statements correctly describe effective nuclear charge (Z_eff)? Select all that apply.

A lower Z_eff makes a given electron easier to remove.

A lower Z_eff is due to the loss of a proton from the nucleus.

The effective nuclear charge is lowered by electron-electron repulsions.

Nuclear charge is only lowered by inner electrons?

Back 33

A lower Z_eff makes a given electron easier to remove.

The effective nuclear charge is lowered by electron-electron repulsions.

Front 34

The energy required for the complete removal of 1 mol of electrons from 1 mol of gaseous atoms or ions is called _____ energy. For a neutral element this energy is a measure of how easily the element forms an ion with a _____ charge.

Back 34

ionization

positive

Front 35

For electronic sublevels within the same principal energy level, in general a higher nuclear charge _____ nucleus-electron attractions and therefore _____ sublevel energies.

Back 35

increases

decreases

A higher nuclear charge increases nucleus-electron attractions thus stabilizing the atom and decreasing sublevel energies.

Front 36

When it comes to atomic radii...

Back 36

Atomic size does not change consistently within a period for transition metals.

The atomic radius of main-group elements decreases across a period.

Atomic radii generally increase as n increases.

Front 37

List the following species in order of increasing radius, with the species with the smallest radius at the top of the list. P3-, Li+, Cl, Cl-, S2-

Back 37

Li+

Cl

Cl-

S2-

P3-

Front 38

Second ionization energies are always _____ than first ionization energies because the remaining electrons are attracted _____ strongly as the positive charge on the ion increases. A large jump ion ionization energies is always observed after the _____ electrons have been removed.

Back 38

higher

more

valence

Front 39

Mg2+, Na+, and F- all have the same electron configuration as Ne, and are described as being _____ with Ne and with each other.

Back 39

isoelectronic

Front 40

Arrange the following elements in order of increasing atomic size, starting with the smallest atom at the top of the list.

Back 40

S

Br

Se

I

Front 41

Metallic behavior...

Back 41

has a tendency to lose electrons and form cations.

It also has high electrical and thermal conductivity.

Front 42

A condensed electron configuration includes the element symbol of the _____ gas that is _____ to the relevant element in square brackets, followed by the configuration of the energy level being filled.

Back 42

noble

prior

Front 43

The Pauli _____ principle guarantees that no two electrons in the same atom have the same quantum number of description. This means that the maximum number of electrons that can be accommodated by any orbital is _____.

Back 43

exclusion

two

Front 44

Which of the following species are isoelectronic with each other? Mg2+, Ar, Cd2+, Br-, Sr2+

Back 44

Br-, Sr2+

Br- and Sr2+ are both isoelectronic with Kr. They are therefore isoelectronic with each other.

Front 45

Which sublevels may be utilized in constructing a partial orbital diagram for a Period 3 element?

3s, 3p, 3d, 2d

Back 45

3s & 3p

Front 46

For any element in the periodic table, the _____ number gives the n value of the _____ principal energy level containing electrons. For main-group elements only, the A _____ number is always equal to the number of valence electrons.

Back 46

period

highest

group

Front 47

An atom of vanadium (Z=23) in its ground state has _____ valence electrons.

Back 47

5

Front 48

Rank the following elements in order of increasing metallic character (from least metallic at the top of the list to most metallic at the bottom).

Al, P, Cs, Zn

Back 48

P, Al, Zn, Cs

Front 49

_____ have a high ionization energy and low electron affinity.

Back 49

noble gases

Front 50

_____ have a high ionization energy and high electron affinity.

Back 50

nonmetals

Front 51

_____ have a low ionization energy and low electron affinity.

Back 51

metals

Front 52

When drawing an orbital diagram, orbitals of _____ energy are filled first. By convention, the _____ electron in a given orbital is designated as ↑ and the direction fo the arrow indicates the electron _____.

Back 52

lower

first

spin

Front 53

In general for main-group elements atomic size _____ from left to right across a period and _____ down a group.

Back 53

decreases

increases

Front 54

Describe the shielding effects in a many-electron system.

Back 54

Inner electrons are more effective at shielding outer electrons in the same level.

The shielding effect increases with an increasing number of electrons in a given sublevel.

Shielding reduces the nuclear charge a given electron experiences.

Front 55

Which orbitals are the last orbitals being filled in the actinide series?

5f, 4f, 3f, 7f, 6f

Back 55

5f

Front 56

Ionization energy generally decreases down a group because as the outermost electron moves _____ the nucleus it takes _____ energy to remove it.

Back 56

farther away from

less

Front 57

Group 1A(1) elements tend to _____

Group 7A(17) elements tend to _____

Group 8A(18) elements tend to _____

Back 57

lose electrons

form acidic oxides

be nonreactive

Front 58

Describe trends in the atomic radii of transition elements.

Back 58

- The size decrease across Period 4 is greater than for Periods 5 & 6.

- Across a transition series, atomic size shrinks through the first two or three elements.

Front 59

Electron configuration for selenium (Z=34)

Back 59

[Ar] 4s² 3d¹⁰ 4p⁴

Front 60

Which type of electrons are best at shielding a 3p electron?

3p, 3s, 3d, 2p, 4p

Back 60

2p

Front 61

Which of the following species has a pseudo-noble gas configuration? Select all that apply.

Pb2+, Br-, Al3+, Zn2+, Sn4+

Back 61

Zn2+ & Sn4+

Front 62

Which of these is the correct orbital diagram for the ground state of carbon?

Back 62

A

Front 63

_____ has the shortest distance between the nuclei of atoms in a molecule of the element.

Back 63

covalent radius

Front 64

_____ has half the shortest distance between nuclei of adjacent atoms in a crystal of the element.

Back 64

metallic radius

Front 65

Which of the following statements correctly describe the trends in ionic size?

Back 65

-within an isoelectronic series, size decreases with increasing nuclear charge.

-ionic size increases down a group on the periodic table.

-anions are larger than their parents.

Front 66

Which of the following electron configurations are associated with increased stability?

Back 66

- A full valence shell or level

- A half-filled sublevel

- A filled sublevel

Front 67

Why is the 2s orbital lower in energy than the 2p orbitals?

Back 67

An electron in the 2s orbital spends part of its time "penetrating" very close to the nucleus, lowering its overall energy.

Front 68

A _____ is larger than the parent atom.

Back 68

Anion

Front 69

A _____ is smaller than the parent atom.

Back 69

Cation

Front 70

Which of the following statements correctly describe electron affinity?

Back 70

- The electron affinity is the energy change for the addition of 1 mol of electrons to 1 mol of gaseous atoms or ions.

- Electron affinity measures the tendency of an element to form an anion.

- The overall trend in electron affinities is to increase from left to right across a period.

Front 71

Which set of quantum numbers correctly designates the indicated electron orbital diagram shown?

2, 1, -1, +1/2

2, 1, -1, -1/2

2, 1, +1, -1/2

2, 2, -1, -1/2

Back 71

2, 1, -1, -1/2

Front 72

What are some general trends in electron configurations?

Back 72

- Among main-group elements the outer electron configurations within a group are identical.

- For any principal energy level n, the total number of orbitals possible for that level is equal to n²

- The period number of an element corresponds to the n value of the highest energy level containing electrons.

Front 73

With their low IEs and small EAs, the members of Group 1A(1) and 2A(2) are strong _____ agents. With their high IEs and large EAs, the members of Group 6A(16) and 7A(17) are strong_____agents.

Back 73

reducing

oxidizing

Front 74

A diamagnetic species has...

Back 74

no unpaired electrons.

Front 75

A paramagnetic species has...

Back 75

one or more unpaired electrons.

Front 76

A species that is slightly repelled by a magnetic field is _____.

Back 76

diamagnetic.

Front 77

A species that is attracted to a magnetic field is _____.

Back 77

paramagnetic.

Front 78

By convention, the spin quantum number assigned to the first electron in any given orbital is _____.

Back 78

+1/2

Front 79

Which of the following species exhibit paramagnetism? Fe3+, Ti4+, V3+, Zn2+, C

Back 79

C, V3+, Fe3+

There are two unpaired 2p electrons in C

There are five 3d electrons in Fe3+

There are two unpaired 3d electrons in V3+

Front 80

Which of the following statements correctly describe many-electron atoms?

Back 80

-principal energy levels are split into sublevels.

-the energies of the orbitals in the atom are affected both by the nuclear charge and by the presence of other electrons.

-the fourth quantum number becomes important in describing an individual electron

Front 81

What is the condensed electron configuration for titanium (Z=22)?

Back 81

[Ar] 4s²3d²