Deck 9: The Periodic Table and Some Atomic Properties

Question 1

The actinides refer to what group of elements?

A) s-block elements
B) d-block elements
C) f-block elements of atomic number 58 through 71
D) f-block elements of atomic number 90 through 103
E) p-block elements

Answer 1

f-block elements of atomic number 90 through 103

Question 2

The inner transition elements include the actinides and the lanthanides.

Answer 2

True

Question 3

The electron affinity is the energy for an atom in its standard state to gain an electron.

Answer 3

False

Question 4

The electron affinity is opposite to the ionization energy.

Question 5

Why was Moseley so sure from his X-ray work that there were no other undiscovered elements besides the three that he predicted in the range of atomic numbers 13-79?

A) The rows on the periodic table were filled.
B) The columns of the periodic table were full.
C) All of the possible atomic weights were assigned.
D) All of the integer atomic numbers were assigned.
E) Mendeleev didn't predict any more.

Question 6

A metallic oxide plus water forms an acid.

Question 7

Elements in the first two groups are part of the main-group elements along with which of the following groups?

A) d-block elements
B) s-block elements
C) actinides
D) lanthanides
E) p-block elements

Question 8

Which of the following pairs of elements are classified as metalloids?

A) aluminum and silicon
B) argon and neon
C) arsenic and germanium
D) bromine and sulfur
E) copper and silver

Question 9

Paramagnetic is not the same as magnetic.

Question 10

The ion represented as has:

A) 22 electrons
B) 48 neutrons
C) 26 protons
D) 4 3d electrons
E) 0 4s electrons

Question 11

Ions always adopt the electron configuration of a nobel gas.

Question 12

Moseley used X-rays to determine the atomic mass of each element.

Question 13

The similar chemical behavior of the elements in a given group in the periodic table is best accounted for by the fact that atoms of these elements have:

A) the same number of isotopes
B) the same number of electrons
C) the same number of electrons in the outermost (valence) shell
D) similar nuclear structures
E) the same number of protons

Question 14

An atom with an even number of electrons is always diamagnetic.

Question 15

The covalent radius, metallic radius, and the ionic radius are all equal.

Question 16

Plutonium is among a group of elements referred to as:

A) antinides
B) alkalides
C) chalcocides
D) halides
E) lanthanides

Question 17

Which of the following could never be isoelectronic species?

A) anions of two different elements
B) cations of two different elements
C) an anion and a cation
D) an anion and an atom
E) atoms of two different elements

Question 18

Most transition elements form some monatomic ions that are not:

A) isoelectronic with any other cations
B) isoelectronic with any noble gas
C) isoelectronic with any neutral atom
D) isoelectronic with any other species
E) isoelectronic with any other transition metal ion

Question 19

The ionization energy is the energy for a gaseous atom to lose an electron.

Question 20

The transition elements refer to what group of elements?

A) s-block elements
B) d-block elements
C) actinides
D) lanthanides
E) p-block elements

Question 21

Which of the following isoelectronic species has the largest radius?

A) Ne
B) F-
C) Mg2+
D) Na+
E) O2-

Question 22

Which of the following has the largest atomic radius?

A) Rb
B) Br
C) Mo
D) I

Question 23

Which of the following has the largest radius?

A) Se2-
B) Kr
C) Rb+
D) Br-
E) Y3+

Question 24

Which of the following occurs for the representative elements going left to right across the period?

A) Electronegativity decreases.
B) Atomic size increases.
C) Forces of attraction between electron and nucleus increase because nuclear charge increases.
D) The outer electrons are held more weakly.
E) none of these

Question 25

Which comparison of atomic and/or ionic radii is correct?

A) K+ > K
B) K+ > Ca2+
C) Si > S
D) Kr > Xe
E) Cl > Cl-

Question 26

The effective nuclear charge for sodium is:

A) <11, >10
B) <10, >9
C) <3, >1
D) <1, >0
E) 0

Question 27

A is the sequence Na, Mg, Al, Si, and P. B is the sequence He, Ne, Ar, Kr, and Xe. Which statement below is true?

A) The members of A are decreasing in size.
B) The members of B have larger radii than those of A, respectively. That is He > Na, Ne > Mg, etc.
C) The members of A have larger radii than those of B, respectively.
D) The members of B are decreasing in size.
E) All the members of A are isoelectronic.

Question 28

Choose the INCORRECT statement.

A) Within a given sublevel, each orbital is usually occupied by a single electron before any orbital has two electrons.
B) When a metallic element unites with a nonmetallic element, electrons are lost by atoms of the metal and gained by atoms of the nonmetals.
C) The rare gas atoms complete the filling of the p orbitals.
D) The ionization energy of Ca+ is greater than that for Ca++.
E) Ba2+ is smaller than Ba+.

Question 29

Which of the following statements is INCORRECT?

A) The atomic radius decreases from left to right through a period of elements.
B) Cations are larger than the atoms from which they are formed.
C) The metallic character of elements decreases from left to right through a period of elements.
D) The ionization energy increases from left to right through a period of elements.
E) The atomic radius increases down the periodic table.

Question 30

What is the ground state electron configuration for iron(III)?

A) [Ar]3d5
B) [Ar]4s23d3
C) [Ar]4s13d4
D) [Ar]4s24p3
E) [Ar]4p5

Question 31

Which of the following has the smallest radius?

A) Yb3+
B) Ho3+
C) Nd3+
D) Gd3+
E) Ce3+

Question 32

The first ionization energy for rubidium is +403.0 kJ/mol. How much energy would be required to convert 17.1 g of gaseous rubidium to its gaseous +1 monatomic ion at constant temperature?

A) 185 kJ
B) 80.6 kJ
C) 68.9 kJ
D) 40.4 kJ
E) 34.5 kJ

Question 33

Which of the following has the largest radius?

A) As3-
B) Br
C) Sr2+
D) Cl-
E) Se2-

Question 34

Choose the species from which one electron could most easily be removed.

A) Cl
B) K+
C) K
D) Ca+
E) Ar

Question 35

Which of the following has the largest radius?

A) Cl-
B) Ar
C) Sc3+
D) K+
E) P3-

Question 36

What is the general electronic configuration (where n = principal quantum number) that best describes the halogens as a group?

A) ns1np6
B) ns2np4
C) ns2sp5
D) ns2np6
E) ns2np3

Question 37

Which series of elements shows the smallest difference in atomic radii?

A) Li......F
B) Be......Ra
C) He......Xe
D) C......Pb
E) Sc......Zn

Question 38

Which statement best describes relationships in a modern periodic table?

A) Each transition element is placed in the column of the main group element that it most closely resembles.
B) The fourteen elements in the "lanthanide" series form a new independent period.
C) Metalloids usually are the cations in ionic compounds.
D) Nonmetallic properties tend to predominate for elements at the far right portion of the table.
E) Elements are always arranged in order of increasing atomic weights.

Question 39

Among the alkali metals, cesium reacts more rapidly than sodium because:

A) cesium has more electrons
B) cesium has more neutrons
C) the valence electron of cesium is at a greater average distance from the nucleus
D) cesium has a higher atomic weight
E) cesium has more protons

Question 40

Which ground state electronic configuration will most readily produce an ion with a charge of 2+?

A) 1s22s22p63s23p63d104s2
B) 1s22s22p63s23p64s1
C) 1s22s22p63s23p4
D) 1s22s22p63s23p63d104s24p2
E) 1s2s22p63s23p63d104s24p6

Question 41

Chlorine has a large negative electron affinity. Therefore, chlorine is most likely to:

A) act as an oxidizing agent
B) have a small first ionization energy
C) act as a reducing agent
D) form a basic oxide
E) release electrons readily to other atoms

Question 42

Which of the following has the smallest second ionization energy?

A) Si
B) Mg
C) Al
D) P

Question 43

Choose a basic oxide.

A) MgO
B) CO2
C) Cl2O
D) SO2

Question 44

Which of the following elements form amphoteric oxides?

A) Sn
B) Mg
C) P
D) B
E) Na

Question 45

Which of the following species is most likely to be diamagnetic?

A) Fe
B) I
C) Mn+
D) W3+
E) Zn2+

Question 46

What is the relationship between ionization energy and atomic radii?

A) Energy increases as radii increase.
B) Energy is negative for all large radii.
C) Energy decreases as radii decrease.
D) Energy decreases as radii increase
E) Energy increases as as radii decrease

Question 47

What is the general relationship between electron affinity and atomic radii?

A) Electron affinity becomes more negative as radii increases.
B) Electron affinity becomes more negative as radii decreases.
C) Electron affinity becomes positive as radii decreases.
D) Electron affinity becomes positive as radii increases.
E) The two quantities are unrelated

Question 48

Which of the following elements is likely to have the largest second ionization energy?

A) Na
B) Mg
C) Al
D) Si

Question 49

Why is the electron affinity so positive for the group 12 elements?

A) The added electron would have to go into a new shell.
B) The added electron would have to be added into the half-filled p subshell.
C) The added electron would have to be added into the p subshell.
D) The groups 12 elements are diatomic elements.
E) Electrons can't be added to gases.

Question 50

Which of the following reactions gives a positive value for the electron affinity?

A) S-(g) + e- → S2-(g)
B) O(g) + e- → O-(g)
C) S(g) + e- → S-(g)
D) Br(g) + e- → Br-(g)

Question 51

The first ionization potential for S is lower than the first ionization potential for P because:

A) Hund's rule is violated
B) P has a p3 configuration
C) ionization potentials decrease across a representative period
D) P is to the right of S on the periodic table
E) P is below S on the periodic table

Question 52

Which of the following species is diamagnetic?

A) F-
B) C
C) Al
D) S-
E) Na

Question 53

Why is the electron affinity so positive for the noble gas elements?

A) The added electron would have to go into a new shell.
B) The added electron would have to be added into the half-filled p subshell.
C) The added electron would have to be added into the p subshell.
D) The noble gas elements are diatomic elements.
E) Electrons can't be added to gases.

Question 54

Can metal atoms form negative ions in the gaseous state? Explain.

A) No, an electron cannot be added.
B) No, only a liquid can be ionized.
C) Yes, electrons can be added to a Li half-filled 2s orbital.
D) Yes, electrons can be removed from a Li half-filled 2s orbital.
E) No, the 2s orbital is completely filled.

Question 55

Which comparison of ionization energies is correct?

A) Cs > Na
B) Na > Mg
C) Ca > Mg
D) Ca+ > Ca
E) Ar > He

Question 56

Which of the following has the greatest number of unpaired electrons?

A) Cr2+
B) Ti3+
C) Co2+
D) Ni

Question 57

Why is the electron affinity so positive for the group 2 elements?

A) The added electron would have to go into a new shell.
B) The added electron would have to be added into the half-filled p subshell.
C) The added electron would have to be added into the p subshell.
D) The groups 2 elements are diatomic elements.
E) Electrons can't be added to gases.

Question 58

Which species is diamagnetic?

A) atomic sodium
B) atomic fluorine
C) iron(III) ion
D) calcium(II) ion
E) cobalt(II) ion

Question 59

The boiling point for gallium is 2403°C. The boiling point for thallium is 1457°C. Which of the following would be the predicted boiling point for indium?

A) 3860°C
B) 1287°C
C) 946°C
D) 1930°C
E) 730°C

Question 60

The first ionization potentials for calcium and barium are 589.7 kJ/mol and 502.8 kJ/mol. What is the predicted first ionization potential for strontium?

A) 546.3 kJ/mol
B) 1092.5 kJ/mol
C) 86.9 kJ/mol
D) 435.7 kJ/mol
E) 588 kJ/mol

Question 61

Which of the listed elements is the poorest conductor of both heat and electricity?

A) aluminum
B) bismuth
C) cobalt
D) magnesium
E) phosphorus

Question 62

Which would you expect to have the highest melting point?

A) CF4
B) HI
C) HCl
D) HBr
E) All have the same melting point.

Question 63

Which of the following is an amphoteric oxide?

A) Al2O3
B) Li2O
C) PO3
D) Sc2O3
E) SrO

Question 64

Which of the following has the smallest value of the first ionization energy: Ar, Cs, N, Cu, Rb?

A) Ar
B) Cs
C) N
D) Cu
E) Rb

Question 65

List in order of increasing ionization potential: O, Mg, Rb, S, Si.

A) Si < O < Mg < Rb < S
B) Si < S < Rb < Mg < O
C) Mg < O < Rb < S < Si
D) Rb < Mg < Si < S < O
E) S < Si < Mg < O < Rb

Question 66

List in order of increasing atomic size: F, Na, K, Mg, Ne.

A) K < Mg < Ne < Na < F
B) Ne < Mg < K < Na < F
C) Ne < F < Mg < Na < K
D) Mg < F < Ne < Na < K
E) K < Na < Mg < F < Ne

Question 67

Arrange the following in order of increasing ionization energy: Li, Cs, K.

A) K < Li < Cs
B) Cs < K < Li
C) Li < Cs < K
D) Cs < Li < K
E) K < Cs < Li

Question 68

List in order of increasing ionization energy: Na, K, F, Mg, Ne.

A) Na < K < F < Ne < Mg
B) K < Na < Mg < F < Ne
C) Ne < Mg < F < K < Na
D) F < Mg < Ne < K < Na
E) Ne < Na < Mg < F < K

Question 69

Which of the following has the highest first ionization potential: Sb, I, In, Xe, Rb?

A) Sb
B) I
C) In
D) Xe
E) Rb

Question 70

The energy difference between atomic cesium and its most stable ion, in the gaseous state, is referred to as ________.

A) atomic energy
B) electron affinity
C) entropy of vaporization
D) ionization energy
E) magnetic moment

Question 71

List in order of increasing charge of the most common ion: S, Na, F, Ca, Al

A) S2-, Na-, F+, Ca2+, Al3+
B) Ca2-, F-, Al+, Na2+, S3+
C) F2-, S-, Ca+, Al2+, Na3+
D) S2-, F-, Na+, Ca2+, Al3+
E) Al2-, Ca-, F+, Na2+, S3+

Question 72

List in order of increasing atomic size: Sr, Se, Cs, Ga, In.

A) Se < Ga < In < Sr < Cs
B) Ga < In < Se < Cs < Sr
C) Sr < In < Ga < Se < Cs
D) In < Ga < Cs < Se < Sr
E) Cs < Ga < Se < Sr < In

Question 73

If the formula of an oxide is X2O3, what is the formula of the chloride of X?

A) XCl
B) X3Cl
C) XCl3
D) XCl6
E) X2Cl3

Question 74

From the following data, what is the estimated boiling point of liquid chlorine? argon/bp 87 K bromine/bp 332 K fluorine/bp 86 K sulfur/bp 718 K

A) 525 K
B) 402 K
C) 209 K
D) 148 K
E) 123 K

Question 75

List in order of increasing size: Cl-, Ar, K+, S2-, Ca2+.

A) Ca2+ < K+ < Ar < Cl- < S2-
B) S2- < Cl- < Ar < K+ < Ca2+
C) Ca2+ < S2- < K+ < Ar < Cl-
D) Cl- < Ar < K+ < S2- < Ca2+
E) K+ < S2- < Ar < Cl- < Ca2+

Question 76

The number of valence electrons for atomic potassium is ________.

A) 1
B) 5
C) 6
D) 15
E) 19

Question 77

Which of the following has the highest first ionization potential: K, Ge, Kr, Ca, Br?

A) K
B) Ge
C) Kr
D) Ca
E) Br

Question 78

Which of the following atoms has the smallest atomic radius: Br, K, Fe, Cu, Bi?

A) Br
B) K
C) Fe
D) Cu
E) Bi

Question 79

Which main group atom or ion should be included in the following list? Br-, Se2-, Kr, Sr2+

A) As3-
B) Ar
C) K+
D) S2-

Question 80

List in order of increasing size: K+, Se2-, Cl-, Na+, S2-.

A) Cl- < S2- < K+ < Na+ < Se2-
B) Na+ < K+ < Cl- < S2- < Se2-
C) S2- < Na+ < Cl- < Se2- < K+
D) Cl- < Se2- < K+ < Na+ < S2-
E) K+ < Na+ < Cl- < Se2- < S2-