Chapter 8: Electronic Structure and the Periodic Table

Question 1

valence electrons have the highest …. in an atom, or occupy an …. from a …

Answer 1

principal quantum number; unfilled subshell; lower shell

Question 2

electrons in filled subshells that have lower principal quantum numbers are called

Answer 2

core electrons

Question 3

the orbitals in which the valence electrons reside are called the

Answer 3

valence orbitals

Question 4

valence orbitals include the orbitals of the …., and, if an atom has d or f electrons, the orbitals of any …

Answer 4

highest principal quantum number; partially-filled subshells of lower principal quantum number

Question 5

the periodic table can be divided into four blocks of elements: elements with highest energy electrons in

Answer 5

s,p,d, or f subshells

Question 6

the arrangement of the elements in the periodic table correlates with the

Answer 6

subhsells that hold the electrons in the atom

Question 7

the period number is the same as the …

Answer 7

principal quantum number of the outermost electron

Question 8

elements that have one electron in a new principal shell in the energy level diagram start a

Answer 8

new period on the periodic table

Question 9

the 4s subhsell is lower in energy than the

Answer 9

3d subshell

Question 10

the two columns on the left are the … elements, that is, elements for which the highest energy electrons occupy an .. subshell

Answer 10

s-block; s

Question 11

the six columns on the right are .. elements, the 10 columns in the middle are … elements, and the … elements are at the bottom

Answer 11

p-block; d-block; f-block

Question 12

the …is the value of n for the s or p subshells, the … is the value of n for the d subshells, and the … is the value of n for the f subshell

Answer 12

period number; period number-1; period number-2

Question 13

for ions, electrons of … are removed first. for subshells of the same n level, electrons are removed from the …

Answer 13

highest n value; subshell of highest l value first

Question 14

for d-block transition elements, the …electrons are lost before the … electrons

Answer 14

ns; (n-1)d

Question 15

anions are formed b the addition of

Answer 15

electrons to valence orbitals

Question 16

cations are formed by the loss of … from the orbitals with the

Answer 16

valence electrons; greatest n values

Question 17

an isolectronic species is a group of atoms and ions that contain the

Answer 17

same number of electrons

Question 18

the species in an isoelectronic series have the same

Answer 18

electron configuration

Question 19

an atomic radius is half the distance between

Answer 19

adjacent atoms of the same element in a molecule

Question 20

the ionic radius is the measure of the

Answer 20

size of an ion in an ionic solid

Question 21

an atom is always … than any of its cations

Answer 21

larger

Question 22

the greater the positive charge on the cation of the same element, the … the ionic radius

Answer 22

smaller

Question 23

anions are always … than the neutral atoms

Answer 23

larger

Question 24

because each member of an isoelectronic series has the same number of electrons, the …. determines the size within the series

Answer 24

number of protons in the nucleus

Question 25

increasing the nuclear charge increases the electrostatic attractions that the nucleus exerts on the electrons, causing the

Answer 25

radius of the species to decrease

Question 26

in an isoelectronic series, the species with the largest number of protons in its nucleus has the

Answer 26

smallest radius

Question 27

the radii of atoms ... down any group because of the increase in the ...

Answer 27

increase; principal quantum number of the valence orbitals

Question 28

the size trends of atoms in any given period are determined by the

Answer 28

attraction between the nucleus and the valence electrons

Question 29

the effective nuclear charge, Zeff, is the .... experienced by electrons in a subshell

Answer 29

net positive charge

Question 30

the larger effective nuclear charges increases the

Answer 30

electrostatic attraction of the nucleus for the outermost electrons

Question 31

the radii of atoms ... across a period because of the ...

Answer 31

decrease; increase in effective nuclear charge

Question 32

elements at the bottom left of the table have the ... radii, and those in the upper right are ...

Answer 32

largest; smallest

Question 33

the (n-1)d electrons shield the ns electrons from the additional charge that is added to the nucleus with each additional electron, so the effective nuclear charge on the outer ns electrons

Answer 33

increases only slowly

Question 34

ionization energy is the energy required to ...electrons that are attracted by a large effective nuclear charge, f

Answer 34

remove an electron from a gaseous atom or ion in its electronic ground state.

Question 35

the energy needed to remove the first electron is the ... (...), that needed to remove the second electron is the ...(..), and so forth

Answer 35

first ionization energy (I1); second ionization energy (I2)

Question 36

ionization energies are deterined by the strength of the

Answer 36

interaction between the nucleus and the valence electrons

Question 37

electrons that are atracted by a large effective nuclear charge are ... to remove, whereas weakly attracted electrons are ..

Answer 37

difficult; easily removed

Question 38

ionization energies ... across rows in a period because of the ...

Answer 38

increase; increase in effective nuclear charge

Question 39

the ionization energies are more sensitive than the radii to changes in the

Answer 39

occupied subshells

Question 40

slight breaks in the increasing ionization energies across a period are observed at ..., where electrons first ..., and at ..., where electrons are first ...

Answer 40

group 3; enter the p subshell; group 6; paired in the p subshell

Question 41

(group 3)the slight decrease in the ionization energy trend is explained by the smaller ... of the inner electrons by an np1 electron in comparison with s^2 electrons

Answer 41

penetration

Question 42

(group 6) two electrons in the same p orbital repel each other more considerably than two electrons in different p orbitals, causing a

Answer 42

decrease in the ionization energy

Question 43

in general, ionization energies ... down a group, principally because of...

Answer 43

decrease; size considerations

Question 44

the valence electrons of the heavier elements are ..., so electrostatic attractions are ...

Answer 44

farther from the nucleus; weaker

Question 45

the decrease in ionization energies is not as great as one would expect because the effective nuclear charge that attracts the valence electrons increases from the top to the bottom of the group, partially

Answer 45

canceling the effect

Question 46

the differences between ionization energies of the transition metals in any period are

Answer 46

small

Question 47

the species with the greatest charge in the nucleus fror isoelectronic series has the

Answer 47

greatest ionization energy

Question 48

valence electrons are ... than core electrons

Answer 48

much easier to remove

Question 49

pseudo-noble-gas electron configuration →

Answer 49

[noble gas](n-1)d^10

Question 50

in general, the lowest possible charge found on a transition metal occurs when the ..., leadig to cations with a ...

Answer 50

ns electrons are removed; 2+ charge

Question 51

representative-element metals can lose electrons until the cations attain a

Answer 51

noble-gas or a pseudo-noble-gas electron configuration.

Question 52

electron affinity: energ change when an electron is

Answer 52

added to a gaseous atom to form an anion

Question 53

the eleements with the highest (most favorable) electron affinities are the

Answer 53

group 17 elements

Question 54

group 17 elements have the highest .. in their period and a vacancy in the ... to hold an additional electron and complete a ..

Answer 54

effective nuclear charges; valence p orbitals; valence shell octet

Question 55

.... has oe of the largest electron affinities of all the elements

Answer 55

fluorine

Question 56

electron affinities are generally most favorable for eleents with

Answer 56

high ionization energies

Question 57

because the single electron in the s valence orbital is easily removed for group 1 metals, these elements are

Answer 57

highly reactive

Question 58

each of the alkali metals mits light of a ... whenthe metal or a compound containing the metal is ..., a procedure called a ...

Answer 58

characteristic color; placed in a flame; flame test

Question 59

flame tests are used to determine which elements are present in sampes of ..., ad the intensity of the colors is used to determine the ...

Answer 59

unknown composition (qualtitative analysis); amounts of the elements in the samples (quantitive analysis)

Question 60

in superoxide, oxygen has an oxidation number of

Answer 60

-1/2

Question 61

the reactivity of the group 1 metals .... down the group. their chemistry dis dominated by the formation of ... ions

Answer 61

increases; M+

Question 62

the alkaline earth metals are reactive, but not as reactive as the alkali metals, because group 2 has greater

Answer 62

ionization energies

Question 63

most reactions of group 2 elements leads to the formation of ionic compound in which the two

Answer 63

valence electrons are removed

Question 64

the reactivity of group 2 metlas ... down the group

Answer 64

increases

Question 65

the reactivity of the haogens .. down the grouop. their chemistry is dominated by the formation of ... ions

Answer 65

decreases; X-

Question 66

interhalogens: compounds formed from

Answer 66

two different halogens

Question 67

most of the interhalogens have the general formula ..., where X is one of the .... and n=...

Answer 67

XFn; heavier halogens; 1,3,5