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Unit 1 Retest

Total questions: 25

Worksheet time: 2hrs 25mins

Name
Class
Date
1.

What is the empirical formula for hydrogen peroxide which has a molecular formula of H2O2?

a)

HO

b)

H2O2

c)

H2O

2.

The empirical formula for a compound is CH2 and its relative atomic mass (Ar) is 70. What is its molecular formula? Use the periodic table to help you.

a)

CH2

b)

C5H10

c)

C70H140

3.

What is the percentage yield if the actual yield was 2.4 g and the predicted yield was 3.0 g?

a)

75%

b)

80%

c)

125%

4.
What is the percent by mass of fluorine in CaF2 (gram-formula mass = 78 g/mol)?
a)
24%
b)
49%
c)
51%
d)
65%
5.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
6.

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

a)

1

b)

3

c)

6

d)

2

e)

none of these

7.

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+.

8.
What is this element? 
1s22s22p63s23p6
4s23d104p6
a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
9.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
10.

What is the electron configuration for this PES graph?

a)

1s22s22p63s23p2

b)

1s22s22p63s23p1

c)

1s22s22p63s23p3

d)

1s22s22p63s2

11.

Which element is represented by this PES graph?

a)

argon

b)

potassium

c)

calcium

d)

scandium

12.

The photoelectron spectra above show the energy required to remove a 1s electron from a nitrogen atom and from an oxygen atom. Which of the following statements best accounts for the peak in the upper spectrum being to the right of the peak in the lower spectrum?

a)

Nitrogen atoms have a half-filled p subshell.

b)

There are more electron-electron repulsions in oxygen atoms than in nitrogen atoms.

c)

Electrons in the p subshell of oxygen atoms provide more shielding than electrons in the p sub shell of nitrogen atoms.

d)

Nitrogen atoms have a smaller nuclear charge than oxygen atoms.

13.

A sample containing atoms of C and F was analyze using x-ray photoelectron spectroscopy. The portion of the spectrum showing the 1s peaks for atoms of two elements is shown above. Which of the following correctly identifies the 1s peak for the fluorine atoms and provides an appropriate explanation?

a)

Peak X, because F has a smaller first ionization energy than C has.

b)

Peak X, because F has a greater nuclear charge than C has.

c)

Peak Y, because F is more electronegative than C is.

d)

Peak Y, because F has a smaller atomic radius than C has.

14.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
15.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
16.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
17.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
18.
The minimum energy required to remove an electron from the ground state of an atom
a)
electron configuration
b)
energy levels
c)
ionization energy
d)
ionic bond
19.

Why does Cs have a larger radius than Na?

a)

It has more energy levels

b)

It has fewer energy levels

c)

It has a more effective nuclear charge

d)

It has a less effective nuclear charge

20.

Why does Ca have a larger radius than Se?

a)

It has more energy levels

b)

It has fewer energy levels

c)

It has a more effective nuclear charge

d)

It has a less effective nuclear charge

21.

What is effective nuclear charge?

a)

The charge that effects the mass of the atom.

b)

The charge that the protons feel from the rest of the atom.

c)

The charge felt by the valence electrons.

d)

The charge felt by the core electrons.

22.
The concept of shielding happens because of
a)
attraction between nucleus and valence electrons
b)
attraction between nucleus and core electrons
c)
repulsion between valence electrons and other valence electrons
d)
repulsion between core electrons and valence electrons
23.

Mg2+ and O2- create...

a)

Mg2O3

b)

MgO2

c)

MgO

d)

Mg2O

24.
What is the correct formula for magnesium bromide?
Magnesium = Mg
Bromine = Br
a)
MgBr
b)
MgBr2
c)
Mg2Br
d)
Mg2Br4
25.

What holds ionic compounds together?

a)

electronegativity

b)

electrostatic attraction

c)

static forces

d)

glue electrons

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