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AP Chem Unit 1 Review (Atomic Structure and Properties)

Total questions: 45

Worksheet time: 2hrs 15mins

Name
Class
Date
1.

Which of the following is the most electronegative element?

a)

O

b)

La

c)

Rb

d)

Mg

e)

N

2.

Which element exhibits the greatest number of different oxidation states?

a)

O

b)

La

c)

Rb

d)

Mg

e)

N

3.

Which of the following elements has the smallest ionic radius for its most commonly found ion?

a)

O

b)

La

c)

Rb

d)

Mg

e)

N

4.

The energy required to convert a ground-state atom in the gas phase to a gaseous positive ion

a)

activation energy

b)

free energy

c)

ionization energy

d)

kinetic energy

e)

lattice energy

5.

The energy change that occurs in the conversion of an ionic solid to widely separated gaseous ions.

a)

activation energy

b)

free energy

c)

ionization energy

d)

kinetic energy

e)

lattice energy

6.

Which of the following is a gas in its standard state at 298 K?

a)

Lithium

b)

Nickel

c)

Bromine

d)

Uranium

e)

Fluorine

7.

The elements in which of the following have most nearly the same atomic radius?

a)

Be, B, C, N

b)

Ne, Ar, Kr, Xe

c)

Mg, Ca, Sr, Ba

d)

C, P, Se, I

e)

Cr, Mn, Fe, Co

8.

A solution is known to contain an inorganic salt of a one of the following elements. The solution is colorless. The solution contains a salt of

a)

Cu

b)

Mn

c)

Fe

d)

Ni

e)

Zn

9.

Which two subatomic particles are in the nucleus?

a)

Protons and Neutrons

b)

Protons and Electrons

c)

Neutrons and Electrons

10.
 After the atom is ionised, it then requires more energy to remove a second electron because the second electronis nearer the nucleus.
a)
False
b)
True
c)
Not sure
11.
Only one electron can be removed from the atom, as it then has a stable electronic configuration.
a)
True
b)
False
c)
Not sure
12.
What elements have zero electronegativity?
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
13.

Which equation correctly describes the first ionization energy of X?

a)

X --> X- + e-

b)

X --> X+ + e-

c)

X --> X- + e+

d)

X + e- --> X-

e)

X + e- --> X+

14.

Which of the following would have the largest ionization energy?

a)

Na

b)

Al

c)

Mn

d)

N

e)

Pd

15.

Which of the following would have the smallest ionization energy?

a)

K

b)

P

c)

S

d)

Ca

e)

Mg

16.

Place the following elements in order of increasing ionization energy: Na, O, Mg, Ne, K

a)

Ne, O, Mg, Na, K

b)

Mg, Na, O, K, Ne

c)

K, Mg, Na, O, Ne

d)

K, Na, Mg, O, Ne

17.

Successive ionization energies for an element in Period 4 were determined experimentally and found to be: IE1=600 kJ/mol, IE2=1800 kJ/mol, IE3=2700 kJ/mol, IE4=11,600 kJ/mol and IE5=15,000 kJ/mol. What element is this?

a)

germanium

b)

selenium

c)

gallium

d)

silicon

e)

phosphorous

18.

Using electron configuration and your knowledge of ionization energy, which would you expect to have a higher second ionization energy: Na or Mg?

a)

Na

b)

Mg

c)

Both would be expected to have the same second ionization energy

d)

Cannot be determined

19.

All of the halogens in their elemental form at 25oC and 1 atm are

a)

conductors of electricity

b)

diatomic molecules

c)

odorless

d)

colorless

e)

gases

20.

All alkaline earth metals have the following number of valence electrons:

a)

1

b)

3

c)

6

d)

2

e)

none of these

21.

Ti has __________ in its d orbital.

a)

one electrton

b)

two electrons

c)

three electrons

d)

four electrons

e)

none of these

22.

Order the elements S, Cl, and F in terms of increasing ionization energy.

a)

S, Cl, F

b)

Cl, F, S

c)

F, S, Cl

d)

F, Cl, S

e)

S, F, Cl

23.

Order the elements S, Cl, and F in terms of increasing atomic radii.

a)

S, Cl, F

b)

Cl, F, S

c)

F, S, Cl

d)

F, Cl, S

e)

S, F, Cl

24.

Which of the following atoms would have the largest second ionization energy?

a)

Mg

b)

Cl

c)

S

d)

Ca

e)

Na

25.

Choose the element with the highest ionization energy.

a)

Na

b)

Mg

c)

Al

d)

P

e)

S

26.

Consider the ionization (IE) of the magnesium atom. Which of the following is true?

a)

The IE of Mg is lower than that of Na.

b)

The IE of Mg is lower than that of Ne.

c)

The IE of Mg is lower than that of Be.

d)

The IE of Mg is higher than that of Ca.

e)

The IE of Mg is lower than that of Mg+.

27.

Of the following elements, which is most likely to form a negative ion with a charge of 1-?

a)

Ba

b)

Ca

c)

Si

d)

P

e)

Cl

28.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
29.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
30.
What is the electron configuration of Sulfur  using noble gas method
a)
[Ne]3s1
b)
[Ne]3s23p3
c)
[Ne]3s23p4
31.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
32.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
33.
What is the noble gas configuration for phosphorus?
a)
[Ar] 3p5
b)
[He] 3s2 3p5
c)
[Ne] 3s2 3p3
d)
[Na] 3s2 3p5
34.
Identify the element whose electron configurations ends with 5p3
a)
As
b)
Te
c)
Sb
d)
Sn
35.
Which of the following statements is true about the 3s and the 4s sublevels?
a)
These sublevels have the same energy
b)
These sublevels are the same distance from the nucleus
c)
These sublevels hold different amounts of electrons
d)
These sublevels have the same shape
36.
I am an element in the 3rd row of the periodic table...I have one unpaired electron in my last sublevel...I have 3 valence electrons...who am I?
a)
Na
b)
Al
c)
Cl
d)
Ar
37.

Which peak corresponds to the 1s orbital?

a)

1.06

b)

1.95

c)

13.5

d)

18.7

e)

208

38.

effective nuclear charge of an atom is primarily affected by

a)

inner electrons

b)

outer electrons

c)

nuclear charge

d)

electron distribution

39.

Within a family such as the alkali metals, the ionic radius (a)   as the atomic number increases

40.

The radius of the chlorine atom is (a)   than the radius of the chloride ion.

41.

Which of the following is NOT isoelectronic with the other species?

a)

S2-

b)

Br-

c)

Kr

d)

Sr2+

42.

Which of the following subshells has the lowest energy?

a)

4d

b)

5s

c)

5p

d)

5f

43.

What is ionization energy?

a)

How well an atom attracts electrons in a chemical bond

b)

The relative size of an atom

c)

An atom that has gained or lost an electron

d)

The amount of energy it takes to remove an electron from the valence shell of an atom

44.

Which element has electrons in the greatest number of subshells when it is in its ground state?

a)

C

b)

Na

c)

Ar

d)

Fe

45.

Which element could #3 be based on ionization energy?

a)

Na

b)

Mg

c)

Al

d)

Si

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