Deck 7: Periodic Properties of the Elements

Question 1

The effective nuclear charge of an atom is primarily affected by ________.

A)inner electrons
B)outer electrons
C)nuclear charge
D)electron distribution
E)orbital radial probability

Answer 1

inner electrons

Question 2

Screening of the nuclear charge by core electrons in atoms is ________.

A)less efficient than that by valence electrons
B)more efficient than that by valence electrons
C)essentially identical to that by valence electrons
D)responsible for a general decrease in atomic radius going down a group
E)both essentially identical to that by valence electrons and responsible for a general decrease in atomic radius going down a group

Answer 2

more efficient than that by valence electrons

Question 3

Of the following,which gives the correct order for atomic radius for Mg,Na,P,Si and Ar?

A)Mg > Na > P > Si > Ar
B)Ar > Si > P > Na > Mg
C)Si > P > Ar > Na > Mg
D)Na > Mg > Si > P > Ar
E)Ar > P > Si > Mg > Na

Answer 3

Na > Mg > Si > P > Ar

Question 4

Atomic radius generally increases as we move ________.

A)down a group and from right to left across a period
B)up a group and from left to right across a period
C)down a group and from left to right across a period
D)up a group and from right to left across a period
E)down a group; the period position has no effect

Question 5

Of the choices below,which gives the order for first ionization energies?

A)Cl > S > Al > Ar > Si
B)Ar > Cl > S > Si > Al
C)Al > Si > S > Cl > Ar
D)Cl > S > Al > Si > Ar
E)S > Si > Cl > Al > Ar

Question 6

Which of the following is an isoelectronic series?

A)B^5-, Si^4-, As^3-, Te^2-
B)F^-, Cl^-, Br^-, I^-
C)S, Cl, Ar, K
D)Si^2-, P^2-, S^2-, Cl^2-
E)O^2-, F^-, Ne, Na⁺

Question 7

________ have the lowest first ionization energies of the groups listed.

A)Alkali metals
B)Transition elements
C)Halogens
D)Alkaline earth metals
E)Noble gases

Question 8

Which compound has the smallest ionic separation?

A)NaCl
B)NaBr
C)NaI
D)NaF
E)KF

Question 9

Which of the following correctly represents the third ionization of gallium?

A)Ga (g)→ Ga⁺ (g)+ e^-
B)Ga⁺ (g)→ Ga²⁺ (g)+ e^-
C)Ga^2- (g)+ e^- → Ga^3- (g)
D)Ga²⁺ (g)→ Ga³⁺ (g)+ e^-
E)Ga⁺ (g)+ e^- → Ga²⁺ (g)

Question 10

The atomic radius of main-group elements generally increases down a group because ________.

A)effective nuclear charge increases down a group
B)effective nuclear charge decreases down a group
C)effective nuclear charge zigzags down a group
D)the principal quantum number of the valence orbitals increases
E)both effective nuclear charge increases down a group and the principal quantum number of the valence orbitals increases

Question 11

Which equation correctly represents the first ionization of calcium?

A)Ca (g)→ Ca⁺ (g)+ e^-
B)Ca (g)→ Ca^- (g)+ e^-
C)Ca (g)+ e^- → Ca^- (g)
D)Ca^- (g)→ Ca (g)+ e^-
E)Ca⁺ (g)+ e^- → Ca (g)

Question 12

Electrons in the 1s subshell are much closer to the nucleus in Ar than in He due to the larger ________ in Ar.

A)nuclear charge
B)paramagnetism
C)diamagnetism
D)Hund's rule
E)azimuthal quantum number

Question 13

Rank the following in terms of decreasing first ionization energies?

A)Ne > O > N > Be > B
B)Ne > N > O > B > Be
C)Ne > O > N > B > Be
D)Ne > N > O > Be > B
E)B > Be > O > N > Ne

Question 14

Of the following,which gives the correct order for atomic radius for Ca,K,As,Ge and Kr?

A)Ca > K > As > Ge > Kr
B)Kr > Ge > As > K > Ca
C)Ge > As > Kr > K > Ca
D)K > Ca > Ge > As > Kr
E)Kr > As > Ge > Ca > K

Question 15

Which of the following correctly represents the third ionization of aluminum?

A)Al²⁺ (g)+ e^- → Al⁺ (g)
B)Al (g)→ Al⁺ (g)+ e^-
C)Al^2- (g)+ e^- → Al^3- (g)
D)Al²⁺ (g)+ e^- → Al³⁺ (g)
E)Al²⁺ (g)→ Al³⁺ (g)+ e^-

Question 16

Atomic radius generally decreases as we move ________.

A)down a group and from right to left across a period
B)up a group and from left to right across a period
C)down a group and from left to right across a period
D)up a group and from right to left across a period
E)down a group; the period position has no effect

Question 17

In which set of elements would all members be expected to have very similar chemical properties?

A)P, Se, I
B)Cl, Br, Na
C)Si, As, Te
D)Ne, Na, Mg
E)Br, I, At

Question 18

Which isoelectronic series is correctly arranged in order of increasing radius?

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

Question 19

Which of the following correctly represents the first ionization of oxygen?

A)O (g)→ O⁺ (g)+ e^-
B)O⁺ (g)+ e^- → O²⁺ (g)
C)O (g)+ e^- → O^- (g)
D)O^- (g)+ e^- → O^2- (g)
E)O⁺ (g)+ e^- → O (g)

Question 20

In which set of elements would all members be expected to have very similar chemical properties?

A)O, S, Se
B)N, O, F
C)Na, Mg, K
D)S, Se, Si
E)Ne, Na, Mg

Question 21

Of the following elements,________ has the most negative electron affinity.

A)S
B)Cl
C)Se
D)Br
E)I

Question 22

The electron configuration of the atom with the most negative electron affinity is ________.

A)(i)
B)(ii)
C)(iii)
D)(iv)
E)(v)

Question 23

The list that correctly indicates the order of metallic character is ________.

A)B > N > C
B)F > Cl > S
C)Si > P > S
D)P > S > Se
E)Na > K > Rb

Question 24

Sodium is much more apt to exist as a cation than is chlorine.This is because ________.

A)chlorine is a gas and sodium is a solid
B)chlorine has a greater electron affinity than sodium does
C)chlorine is bigger than sodium
D)chlorine has a greater ionization energy than sodium does
E)chlorine is more metallic than sodium

Question 25

Of the following elements,________ has the most negative electron affinity.

A)P
B)Al
C)Si
D)Cl
E)B

Question 26

The electron configuration belonging to the atom with the highest second ionization energy is ________.

A)(i)
B)(ii)
C)(iii)
D)(iv)
E)(v)

Question 27

Which ion below has the largest radius?

A)Cl^-
B)K⁺
C)Br^-
D)F^-
E)Na⁺

Question 28

Of the elements below,________ has the highest melting point.

A)Ca
B)K
C)Fe
D)Na
E)Ba

Question 29

Which of the following species has the smallest ionic radius?

A)Al³⁺
B)Na⁺
C)Mg²⁺
D)S^2-
E)Cl^-

Question 30

Which of the following correctly represents the electron affinity of phosphorus?

A)P (g)→ P⁺ (g)+ e^-
B)P (g)+ e^- → P^- (g)
C)P₄ (g)+ e^- → P^- (g)
D)P₄ (g)+ 4e^- → 4P^- (g)
E)P⁺ (g)+ e^- → P (g)

Question 31

The electron configuration that belongs to the atom with the lowest first ionization energy is ________.

A)(i)
B)(ii)
C)(iii)
D)(iv)
E)(v)

Question 32

Which of the following correctly represents the electron affinity of bromine?

A)Br (g)→ Br⁺ (g)+ e^-
B)Br (g)+ e^- → Br^- (g)
C)Br₂ (g)+ e^- → Br^- (g)
D)Br₂ (g)+ 2e^- → 2Br^- (g)
E)Br⁺ (g)+ e^- → Br (g)

Question 33

In the generation of most anions,the energy change (kJ/mol)that ________ an electron is ________.

A)removes, positive
B)adds, positive
C)removes, negative
D)adds, negative
E)None of the above is correct.

Question 34

Of the following elements,________ has the most negative electron affinity.

A)O
B)K
C)B
D)Na
E)S

Question 35

Which of the following correctly represents the second ionization of calcium?

A)Ca (g)→ Ca⁺ (g)+ e^-
B)Ca⁺ (g)→ Ca²⁺ (g)+ e^-
C)Ca^- (g)+ e^- → Ca^2- (g)
D)Ca⁺ (g)+ e^- → Ca²⁺ (g)
E)Ca⁺ (g)+ e^- → Ca (g)

Question 36

The electron configuration of the atom that is expected to have the least negative electron affinity is ________.

A)(i)
B)(ii)
C)(iii)
D)(iv)
E)(v)

Question 37

Of the elements below,________ is the most metallic.

A)sodium
B)barium
C)magnesium
D)calcium
E)cesium

Question 38

Which of the following has the most metallic character?

A)Al
B)Ca
C)Mg
D)Sr
E)Si

Question 39

Which equation correctly represents the electron affinity of calcium?

A)Ca (g)+ e^- → Ca^- (g)
B)Ca (g)→ Ca⁺ (g)+ e^-
C)Ca (g)→ Ca^- (g)+ e^-
D)Ca^- (g)→ Ca (g)+ e^-
E)Ca⁺ (g)+ e^- → Ca (g)

Question 40

Which of the following correctly represents the second ionization of copper?

A)Cu (g)→ Cu⁺ (g)+ e^-
B)Cu⁺ (g)→ Cu²⁺ (g)+ e^-
C)Cu^- (g)+ e^- → Cu^2- (g)
D)Cu⁺ (g)+ e^- → Cu²⁺ (g)
E)Cu⁺ (g)+ e^- → Cu (g)

Question 41

Which group in the periodic table has the lowest first ionization energy?

A)VIA
B)IA
C)IIIA
D)IIA
E)VIIA

Question 42

Alkali metals tend to be more reactive than alkaline earth metals because ________.

A)alkali metals have lower densities
B)alkali metals have lower melting points
C)alkali metals have greater electron affinities
D)alkali metals have lower ionization energies
E)Alkali metals are not more reactive than alkaline earth metals.

Question 43

Reacting CO₂ with water results in a(n)________ solution.

A)ionic
B)neutral
C)basic
D)acidic
E)CO₂ does not react with water

Question 44

Which of the following metals differ in the number of d-electrons?

A)Fe and Cu
B)Mg and Fe
C)Na and Rh
D)Cs and Ca
E)Ca and Na

Question 45

Alkaline earth metals ________.

A)have the smallest atomic radius in a given period
B)form monoanions
C)form basic oxides
D)exist as triatomic molecules
E)form halides with the formula MX

Question 46

Which one of the following is not true about the alkali metals?

A)They are low density solids at room temperature.
B)They all readily form ions with a +1 charge.
C)They all have 2 electrons in their valence shells.
D)They are very reactive elements.
E)They have the lowest first ionization energies of the elements.

Question 47

The element in the periodic table that looks like a metal,is a poor thermal conductor,and acts as an electrical semiconductor is ________.

A)Sn
B)B
C)As
D)Si
E)Ge

Question 48

Which of the following elements is the most reactive in water?

A)Na
B)Rb
C)Cs
D)Li
E)K

Question 49

Of the following metals,________ exhibits multiple oxidation states.

A)Al
B)Rb
C)Mg
D)Ni
E)Cs

Question 50

Which of the following oxides do not produce an acidic solution when dissolved in water?

A)SO₃
B)P₂O₅
C)CO₂
D)Al₂O₃
E)Cl₂O

Question 51

The difference in metallic character is the smallest between ________.

A)Li and O
B)Rb and F
C)Na and I
D)Rb and Cl
E)Na and Mg

Question 52

All of the following reactions concerning alkali metals are correct except ________.

A)2Na (s)+ 2H₂O (l)→ 2NaOH (aq)+ H₂ (g)
B)Na (s)+ O₂ (g)→ NaO₂ (s)
C)2Na (s)+ H₂ (g)→ 2NaH (s)
D)2Na (s)+ S (s)→ Na₂S (s)
E)2Na (s)+ Cl₂ (g)→ 2NaCl (s)

Question 53

Consider the general valence electron configuration of ns²np⁵ and the following statements: (i)Elements with this electron configuration are expected to form -1 anions.
(ii)Elements with this electron configuration are expected to have large positive electron affinities.
(iii)Elements with this electron configuration are nonmetals.
(iv)Elements with this electron configuration form acidic oxides.
Which statements are true?

A)(i)and (ii)
B)(i), (ii), and (iii)
C)(ii)and (iii)
D)(i), (iii,)and (iv)
E)All statements are true.

Question 54

Consider the following properties of an element: (i)It is solid at room temperature.
(ii)It easily forms an oxide when exposed to air.
(iii)When it reacts with water,hydrogen gas evolves.
(iv)It must be stored submerged in oil.
Which element fits the above description the best?

A)sulfur
B)copper
C)mercury
D)sodium
E)magnesium

Question 55

The reaction of alkali metals with oxygen produce ________.

A)oxides, peroxides, and superoxides
B)peroxides only
C)superoxides only
D)oxides only
E)none of the above

Question 56

The oxide of which element can react with water to give a basic solution?

A)sulfur
B)calcium
C)phosphorus
D)nitrogen
E)carbon

Question 57

Which of the following is not a characteristic of metals?

A)acidic oxides
B)low ionization energies
C)malleability
D)ductility
E)These are all characteristics of metals.

Question 58

Which of the listed oxides is the most acidic?

A)SO₃
B)Na₂O
C)K₂O
D)Al₂O₃
E)MgO

Question 59

Nonmetals can be ________ at room temperature.

A)solid, liquid, or gas
B)solid or liquid
C)solid only
D)liquid only
E)liquid or gas

Question 60

When two elements combine to form a compound,the ________ the difference in metallic character between the two elements,the ________ the likelihood that the compound will be a ________ at room temperature.

A)smaller, greater, solid
B)greater, greater, liquid
C)greater, greater, solid
D)smaller, greater, liquid
E)greater, smaller, solid

Question 61

Which of the following statements is not true for oxygen?

A)The most stable allotrope of oxygen is O₂.
B)The chemical formula of ozone is O₃.
C)Dry air is about 79% oxygen.
D)Oxygen forms peroxide and superoxide anions.
E)Oxygen is a colorless gas at room temperature.

Question 62

________ is a unique element and does not truly belong to any family.

A)Nitrogen
B)Radium
C)Hydrogen
D)Uranium
E)Helium

Question 63

________ is unique among the elements because its electron is not shielded from its nucleus.

A)Cesium
B)Potassium
C)Hydrogen
D)Lithium
E)Sodium

Question 64

Elements in the modern version of the periodic table are arranged in order of increasing ________.

A)oxidation number
B)atomic mass
C)average atomic mass
D)atomic number
E)number of isotopes

Question 65

The alkali metal that is naturally radioactive is ________.

A)rubidium
B)cesium
C)lithium
D)francium
E)sodium

Question 66

Which of the following noble gases is not reactive?

A)xenon and argon
B)helium and neon
C)xenon only
D)xenon, krypton, and argon
E)None of the above are reactive

Question 67

Hydrogen is unique among the elements because ________. 1.It is not really a member of any particular group.
2.Its electron is not at all shielded from its nucleus.
3.It is the lightest element.
4.It is the only element to exist at room temperature as a diatomic gas.
5.It exhibits some chemical properties similar to those of groups 1A and 7A.

A)1, 2, 3, 5
B)1, 2, 3, 4, 5
C)1, 4, 5
D)3, 4
E)2, 3, 4, 5

Question 68

All of the following elements can exist as allotropes except ________.

A)N
B)Ar
C)O
D)S
E)F

Question 69

In nature,the noble gases exist as ________.

A)monatomic gaseous atoms
B)the gaseous fluorides
C)solids in rocks and in minerals
D)alkali metal salts
E)the sulfides

Question 70

All of the halogens ________.

A)exist under ambient conditions as diatomic gases
B)tend to form positive ions of several different charges
C)tend to form negative ions of several different charges
D)exhibit metallic character
E)form salts with alkali metals with the formula MX

Question 71

iodine has a(n)________ density and a(n)________ atomic radius compared to bromine.

A)smaller, greater
B)greater, smaller
C)smaller, smaller
D)greater, greater
E)equal, equal

Question 72

Ozone is a a(n)________ of oxygen.

A)isotope
B)allotrope
C)precursor
D)peroxide
E)free radical

Question 73

The noble gases were,until relatively recently,thought to be entirely unreactive.Experiments in the early 1960s showed that Xe could,in fact,form compounds with fluorine.The formation of compounds consisting of Xe is made possible by ________.

A)the availability of xenon atoms
B)xenon's noble gas electron configuration
C)the stability of xenon atoms
D)xenon's relatively low ionization energy
E)xenon's relatively low electron affinity

Question 74

________ has been shown to form compounds only when it is combined with something with a tremendous ability to remove electrons from other substances.

A)Neon
B)Helium
C)Hydrogen
D)Xenon
E)Oxygen

Question 75

________ is credited with developing the concept of atomic numbers.

A)Dmitri Mendeleev
B)Lothar Meyer
C)Henry Moseley
D)Ernest Rutherford
E)Michael Faraday

Question 76

Which element is solid at room temperature?

A)Cl₂
B)F₂
C)Br₂
D)I₂
E)H₂

Question 77

Which alkaline earth metal will not react with liquid water or with steam?

A)Be
B)Mg
C)Ca
D)Ba
E)They all react with liquid water and with steam.

Question 78

Lithium ion salts were originally found in Seven-Up® drinks.How many electrons does Li atom lose to become an ion?

A)4
B)3
C)0
D)1
E)2

Question 79

Which of the following elements can exist as an allotrope?

A)iron
B)carbon
C)silver
D)silicon
E)neon

Question 80

Lithium ion salts were used to treat manic-depressive illness.Lithium is part of which group in the periodic table?

A)alkali metals
B)noble gases
C)alkaline earth metals
D)halogens
E)chalcogens