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Ap CHemistry Unit 1 Review

Total questions: 38

Worksheet time: 1hrs 3mins

Name
Class
Date
1.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

2.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
3.
Value representing the number of protons in an element
a)
Atomic Mass
b)
Mass Number
c)
Valence Electrons
d)
Atomic Number
4.
Measure mainly of the nuclear particles: protons + neutrons
a)
Subatomic Particles
b)
Atomic Number
c)
Atomic Mass
d)
Gluons
5.
A charged atom
a)
Ion
b)
Isotope
c)
Electron Cloud
d)
Quark
6.
Arrangement of elements organized by atomic number
a)
Electron Cloud 
b)
Periodic Table 
c)
Electron Configuration
d)
None of these
7.
Proposed the Modern Electron Cloud Model of the atom
a)
Schrodinger & Heisenberg
b)
Dalton
c)
Chadwick
d)
Rutherford
8.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
9.
How many neutrons does the isotope below have?     89 36Kr
a)
53
b)
36
c)
89
d)
125
10.
If X is the symbol for an element, which of the following two symbols represent    isotopes of the same element?     I. 7735X  II. 7733X  III. 8137X  IV. 8135 X
a)
I and II
b)
III and IV
c)
I and IV
d)
I and III
11.
How many isotopes are shown in this mass spectrum?
a)
1
b)
84
c)
86
d)
4
12.
How many isotopes of this element are shown in the mass spectrum?
a)
98
b)
7
c)
100
d)
95.9 g/mol
13.
Based on the mass spectrum, which isotope of chlorine is most abundant?
a)
35Cl
b)
37Cl
c)
70Cl
d)
72Cl
14.
The average atomic mass rhenium, Re, is 186.21 amu. If 37.1% of rhenium has mass# = 185, what is the other stable isotope?
a)
Rhenium-183
b)
Rhenium-181
c)
Rhenium-187
d)
Rhenium-189
15.
The ground state is the highest energy state of an atom.
a)
True
b)
False
16.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
17.

If an electron moves from n=4 to n=2 it ____

a)

absorbs energy

b)

releases energy

18.
What is the empirical formula if you have 36.84% nitrogen and 63.16% oxygen?
a)
NO
b)
N2O3
c)
N2O4
d)
N2O5
19.

A 5.00 g sample of a compound consisting of calcium and chlorine contains 1.82 g of calcium and 3.23 g of chlorine. What is the empirical formula?

a)

CaCl2

b)

Ca2Cl4

c)

Ca2Cl2

d)

Ca4Cl2

20.

How many molecules are in 2.5 mol of NaCl?

a)

1.5 x 1024 molecules

b)

1.5 molecules

c)

4.15 molecules

d)

1.5 x 1023 molecules

21.
Calculate the number of atoms in 0.0340 g Zn.
a)
5.200 x 10-4 atoms Zn
b)
3.130 x 1023 atoms Zn
c)
3.130 x 1020 atoms Zn
d)
1 atom Zn
22.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
23.
What is the molecular formula if the empirical formula is C2H5 and the molecular molar mass is 58.14 g/mol?
a)
C2H5
b)
C4H10
c)
C1H2.5
d)
C4H8
24.
What would be the mass of 1.5mol H2O
a)
20
b)
27
c)
32
d)
40
25.
How many particles would be in 8.4 moles of Octane (C8H18)?
a)
5.77 x 1023
b)
5.04 x 1024
c)
5.77 x 1026
d)
5.04 x 1023
26.
How many moles are in 16.94g of water?
a)
16.94 mol H2O
b)
0.9401 mol H2O
c)
305.3 mol H2O
d)
1.063 mol H2O
27.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
28.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
29.
An example of Coulombic Attraction in an atom is between
a)
protons and neutrons
b)
neutrons and electrons
c)
protons and electrons
d)
protons and protons
30.
As the distance between protons and electrons increases, the force of attraction
a)
remains the same
b)
increases
c)
decreases
d)
is not affected
31.
What are the two variables that affect Coulombic Attraction?
a)
Distance  and number of protons
b)
Number of neutrons and number of protons
c)
Number of neutrons and number of electrons
d)
solids or liquids
32.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
33.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
34.
Which electron configuration belongs to Copper (Cu)?
a)
1s2 2s2 2p6 3s2 3p6 4s2 3d8
b)
1s2 2s2 2p6 3s2 3p6 4s2 3d9
c)
1s2 2s2 2p6 3s2 3p6 4s2 3d10
35.

List the following atoms in order of increasing ionization energy: Li, Na, C, O, F.

a)

Li<Na<C<O<F

b)

Na<Li<C<O<F

c)

F<O<C<Li<Na

d)

Na<Li<F<O<C

e)

Na<Li<C<F<O

36.

Of the following transitions in the Bohr hydrogen atom, the __________ transition results in the emission of the highest-energy photon.

a)

n = 6 ¬ n = 1

b)

n = 1 ¬ n = 6

c)

n = 3 ¬ n = 6

d)

n = 6 ¬ n = 3

37.

An example of an electron configuration of a transition metal is __________.

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1

b)

1s2 2s2 2p6 3s2 3p5

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d8

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6

e)

1s2 2s2 2p4 3s1

38.

Identify the element based on the Photoelectron spectrum provided.

a)

Hydrogen

b)

Helium

c)

Sodium

d)

Magnesium

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