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Periodic Properties

By MikejacynS1 Aug 20, 2013 1734 Words
LAREDO COMMUNITY COLLEGE
Science Department

CHEM 1411-1412Practice Test Ch. 7Periodic PropertiesNewton Name

Instructions: Circle the letter of the BEST answer(s). Some questions may have multiple answers; be sure to include all correct answers. Each correct question is worth two (2) points.
1)

__________ is credited with developing the concept of atomic numbers. A)

Lothar Meyer
B)

Ernest Rutherford
C)

Michael Faraday
D)

Dmitri Mendeleev
E)

Henry Moseley

2)

Elements in the modern version of the periodic table are arranged in order of increasing __________. A)

oxidation number
B)

atomic mass
C)

atomic number
D)

number of isotopes
E)

average atomic mass

3)

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

diamagnetism
B)

azimuthal quantum number
C)

paramagnetism
D)

Hund's rule
E)

nuclear charge

4)

Atomic radius generally increases as we move __________.
A)

up a group and from left to right across a period
B)

down a group and from right to left 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

5)

Screening by the valence electrons in atoms is __________.
A)

more efficient than that by core electrons
B)

less efficient than that by core electrons
C)

responsible for a general increase in atomic radius going across a period D)

essentially identical to that by core electrons
E)

both more efficient than that by core electrons and responsible for a general increase in atomic radius going across a period

6)

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 zigzags down a group
C)

effective nuclear charge decreases 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

7)

Which of the following correctly lists the five atoms in order of increasing size (smallest to largest)? A)

O < F < S < Mg < Ba
B)

O < F < S < Ba < Mg
C)

F < O < S < Mg < Ba
D)

F < S < O < Mg < Ba
E)

F < O < S < Ba < Mg

Consider the following electron configurations to answer the questions that follow:

(i)[Kr]
(ii)[Ne]
(iii)[Ar]
(iv)[Ne]
(v)[Ar]

8)

The electron configuration of the atom that is expected to form a stable -2 ion is __________. A)

(i)

B)

(ii)

C)

(iii)

D)

(iv)

E)

(v)

9)

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

Al > Si > S > Cl > Ar
B)

Cl > S > Al > Si > Ar
C)

S > Si > Cl > Al > Ar
D)

Cl > S > Al > Ar > Si
E)

Ar > Cl > S > Si > Al

10)

__________ have the lowest first ionization energies of the groups listed. A)

Noble gases
B)

Alkali metals
C)

Halogens
D)

Alkaline earth metals
E)

Transition elements

11)

Which of the following has the largest second ionization energy? A)

K

B)

Ca

C)

Ga

D)

Ge

E)

Se

12)

Which of the following correctly represents the second ionization of aluminum? A)

(g) →_ (g) +
B)

Al (g) →_ (g) +
C)

Al- (g) + →_ (g)
D)

(g) + →_ (g)
E)

(g) + →_ Al (g)

13)

Which ion in the isoelectronic series below has the largest radius in a crystal? A)

B)

C)

D)

E)

14)

Which of the following sets contains species that are isoelectronic? A)

, , Ar
B)

, ,
C)

O, F, Ne
D)

, , Ne
E)

Na, Mg, Al

15)

__________ is isoelectronic with argon and __________ is isoelectronic with neon. A)

,

B)

,

C)

,

D)

F+,

E)

,

16)

The __________ have the most negative electron affinities.
A)

transition metals
B)

alkali metals
C)

alkaline earth metals
D)

halogens
E)

chalcogens

17)

In general, as you go across a period in the periodic table from left to right: (1) the atomic radius __________;
(2) the electron affinity becomes __________ negative; and (3) the first ionization energy __________.
A)

decreases, decreasingly, decreases
B)

decreases, decreasingly, increases
C)

decreases, increasingly, increases
D)

increases, increasingly, decreases
E)

increases, increasingly, increases

18)

Chlorine is much more apt to exist as an anion than is sodium. This is because __________. A)

chlorine is more metallic than sodium
B)

chlorine is bigger than sodium
C)

chlorine has a greater electron affinity than sodium does
D)

chlorine has a greater ionization energy than sodium does
E)

chlorine is a gas and sodium is a solid

19)

Sodium is much more apt to exist as a cation than is chlorine. This is because __________. A)

chlorine is bigger than sodium
B)

chlorine is a gas and sodium is a solid
C)

chlorine has a greater ionization energy than sodium does
D)

chlorine is more metallic than sodium
E)

chlorine has a greater electron affinity than sodium does

Consider the following electron configurations to answer the questions that follow:

(i)1 2 2 3
(ii)1 2 2 3
(iii)1 2 2 3 3
(iv)1 2 2 3 3
(v)1 2 2 3 3

20)

The electron configuration of the atom with the most negative electron affinity is __________. A)

(i)

B)

(ii)

C)

(iii)

D)

(iv)

E)

(v)

21)

The electron configuration of the atom that is expected to have a positive electron affinity is __________. A)

(i)

B)

(ii)

C)

(iii)

D)

(iv)

E)

(v)

22)

Of the elements below, __________ is the most metallic.
A)

cesium

B)

calcium

C)

barium

D)

magnesium

E)

sodium

23)

Which one of the following is a metalloid?
A)

Pb

B)

Ge

C)

S

D)

Br

E)

C

24)

Element M reacts with chlorine to form a compound with the formula M. Element M is more reactive than magnesium and has a smaller radius than barium. This element is __________. A)

Be

B)

K

C)

Sr

D)

Ra

E)

Na

25)

Of the following metals, __________ exhibits multiple oxidation states. A)

Cs

B)

Na

C)

V

D)

Ca

E)

Al

26)

Metals can be __________ at room temperature.
A)

liquid only
B)

solid only
C)

liquid or gas
D)

solid or liquid
E)

solid, liquid, or gas

27)

Nonmetals can be __________ at room temperature.
A)

solid only
B)

solid, liquid, or gas
C)

liquid or gas
D)

liquid only
E)

solid or liquid

28)

Most of the elements on the periodic table are __________.
A)

gases

B)

metals

C)

metalloids

D)

liquids

E)

nonmetals

29)

Na reacts with element X to form an ionic compound with the formula X. Ca will react with X to form __________. A)

Ca

B)

X

C)

CaX

D)

E)

30)

Elemental sodium is prepared commercially by __________.
A)

reaction of sulfuric acid with brine
B)

pyrolysis of limestone
C)

roasting of galena
D)

electrolysis of molten NaCl
E)

electrolysis of seawater

31)

Alkali metals tend to be more reactive than alkaline earth metals because __________. A)

alkali metals have lower ionization energies
B)

alkali metals have lower melting points
C)

alkali metals have lower densities
D)

alkali metals have greater electron affinities
E)

alkali metals are not more reactive than alkaline earth metals

32)

__________ is a unique element and does not truly belong to any family. A)

Radium

B)

Uranium

C)

Hydrogen

D)

Nitrogen

E)

Helium

33)

Of the following statements, __________ is not true for oxygen. A)

Dry air is about 79% oxygen.
B)

Oxygen forms peroxide and superoxide anions.
C)

The chemical formula of ozone is .
D)

Oxygen is a colorless gas at room temperature.
E)

The most stable allotrope of oxygen is .

34)

All of the halogens __________.
A)

exhibit metallic character
B)

exist under ambient conditions as diatomic gases
C)

tend to form negative ions of several different charges
D)

form salts with alkali metals with the formula MX
E)

tend to form positive ions of several different charges

35)

In nature, the noble gases exist as
A)

alkali metal salts
B)

solids in rocks and in minerals
C)

the gaseous fluorides
D)

monatomic gaseous atoms
E)

the sulfides

36)

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, 4, 5

B)

2, 3, 4, 5

C)

3, 4

D)

1, 2, 3, 5

E)

1, 4, 5

37)

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)

xenon's relatively low ionization energy
B)

xenon's noble gas electron configuration
C)

xenon's relatively low electron affinity
D)

the instability of xenon atoms
E)

the stability of xenon atoms

38)

Of the following elements, which have been shown to form compounds?

helium neon argon krypton xenon
A)

xenon and argon
B)

xenon only
C)

xenon and krypton
D)

xenon, krypton, and argon
E)

None of the above can form compounds.

39)

Xenon has been shown to form compounds only when it is combined with __________. A)

another noble gas
B)

an alkaline earth metal
C)

something with a tremendous ability to donate electrons to other substances D)

an alkali metal
E)

something with a tremendous ability to remove electrons from other substances

40)

The only noble gas that does not have the nn valence electron configuration is __________. A)

neon
B)

helium
C)

radon
D)

krypton
E)

All noble gases have the nn valence electron configuration.

1)

E

2)

C

3)

E

4)

B

5)

B

6)

D

7)

C

8)

C

9)

E

10)

B

11)

A

12)

A

13)

A

14)

A

15)

B

16)

D

17)

C

18)

C

19)

C

20)

E

21)

B

22)

A

23)

B

24)

C

25)

C

26)

D

27)

B

28)

B

29)

E

30)

D

31)

A

32)

C

33)

A

34)

D

35)

D

36)

D

37)

A

38)

D

39)

E

40)

B

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