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Chemistry Midterm

Total questions: 75

Worksheet time: 2hrs 43mins

Name
Class
Date
1.
A mixture that is NOT evenly distributed is called ....
a)
Compounded
b)
Homogenous
c)
Heterogenous
d)
Salty
2.
Are made from a combination of 2 or more elements in a constant ratio...
a)
Atome
b)
Mixture
c)
Compounds
d)
Elements
3.
What is the formula for density?
a)
density = mass x volume
b)
density = mass / volume
c)
density = mass + volume
d)
density = mass - volume
4.
What units can be used to express density?
a)
g/mL
b)
grams
c)
millimeters
d)
milliliters
5.
A bar of copper has a mass of 216g and a volume of 24cm3. What is the density of copper?  
a)
9g/cm3
b)
.11g/cm3
c)
5184g/cm3
d)
322mL
6.
What kind of properties can only be observed when a substance changes into a different substance?
a)
physical properties
b)
chemical properties
7.
Properties that can be observed without changing the identity of the substance.
a)
Physical
b)
Chemical
8.
Example for chemical property
a)
color
b)
hardness
c)
toxicity
d)
solubility
9.
Example for physical property
a)
melting point
b)
flammability
c)
reactivity 
d)
combustion
10.
Example for chemical property
a)
malleability
b)
texture
c)
combustion
d)
sour taste
11.

Rutherford discovered what subatomic particle through his experimentation?

a)

The proton

b)

The neutron

c)

The electron

d)

The quark

12.

Thomson concluded that cathode rays have a negative charge. Why did his experiment lead him to this conclusion?

a)

Opposite charges attract

b)

Like charges attract

c)

Opposite charges repel

d)

Like charges repel

13.

In his experiment, Rutherford concluded that atoms have a nucleus because

a)

most of the particles went straight through the foil.

b)

some of the particles were deflected near the front of the screen.

c)

some of the particles were deflected back towards the alpha source.

d)

not enough information is given.

14.
Isotopes of the same element have different ____________. 
a)
 numbers of protons  
b)
numbers of electrons
c)
 symbols 
d)
numbers of neutrons
15.
The atomic number of an atom or ion refers to the number of:
a)
neutrons
b)
protons
c)
nucleons
d)
electrons
16.
How many electrons does potassium K contain? (click to see image)
a)
19
b)
39
c)
20
d)
40
17.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
18.
which explanation of this notation is correct?
a)
 12 is proton #
b)
6 tells you there are 6 neutrons
c)
6 tells you there are 6 protons
d)
12 is not a mass # here
19.

What do these isotopes of carbon all have in common?

a)

neutrons & mass number

b)

atomic number and neutrons

c)

atomic number and electrons

d)

protons, atomic number, and mass number

20.
Which particles are found in the nucleus
a)
electrons and protons
b)
neutrons and protons
c)
neutrons and electrons
d)
footballs and soccer balls
21.

Which statement is INCORRECT use of mole measurement?

a)

one mole of calcium is 40.01 grams.

b)

one mole of calcium is equals to 6.02 x 1023 atoms

c)

two moles of CaCl2 is equal to 6.02 x 1023 molecules

d)

two moles of KI is equals to 166g

22.

When compared, a mole of oxygen and a mole of sulfur, how many atoms each has?

a)

oxygen has 16 grams of atoms

b)

sulfur has 32.06 grams of atoms

c)

both contains 6.02 x 1023 atoms

d)

A

23.
What is the mass of 3.01 x 1022 atoms of magnesium?
a)
1.22 grams
b)
1.215 grams
c)
1.2 grams
d)
1.22x1046 grams
24.

What element is represented in this Bohr Model?

a)

Carbon

b)

Hydrogen

c)

Aluminum

d)

Lithium

25.
What is the name of this element?
a)
Lithium
b)
Boron
c)
Carbon
d)
Neon
26.
An element with five valence electrons is
a)
phosphorus
b)
oxygen
c)
beryllium
d)
rubidium
27.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
28.

When can atoms emit photons?

a)

When the electron is in the ground state

b)

When the electron is in the excited state

c)

When an electron is going from the ground state to the excited state

d)

When an electron is going from the excited state to the ground state

29.

Which energy state has more energy?

a)

Ground State

b)

Excited State

30.

What is happening in the picture

a)

An atom is absorbing energy to go to a higher state

b)

An atom is emitting a photon to go to a lower state

c)

The atom is losing an electron

d)

The atom is losing a proton

31.
Why did the alpha particle (positively charged particle) sometimes bounce back when hitting the gold foil.
a)
hit neutron in nucleus and they repelled alpha particle
b)
hit proton in nucleus and they repelled alpha particle
c)
hit electrons in electron shells and they repelled alpha particle
32.
What did Bohr add to the model of the atom?
a)
electrons found in specific orbits around nucleus 
b)
 electrons found in nucleus
c)
discovered electron
d)
neutrons found in nucleus
33.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
34.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
35.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
36.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
37.

This is a correct dot diagram for nitrogen (N)

a)

true

b)

false

38.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

39.

What is the goal of the Lewis Dot Structure?

a)

To determine the electron position.

b)

To show the element's valence electrons & bonding capabilities.

c)

To find the atomic mass of an element.

d)

To search for the number of electrons in an individual atom.

40.

Which of the following is NOT a property of ionic compounds?

a)

They conduct electricity when molten

b)

They conduct electricity when in solution

c)

They have high boiling points

d)

They are insoluble in water

41.
A(n) _________ is an ion with a positive (+) charge.
a)
anion
b)
cation
c)
ion
d)
solute
42.
When an atom loses an electron, it becomes a:
a)
positive ion
b)
negative ion
c)
neutral ion
d)
neutral atom
43.
Which of the following is a characteristic property of ionic compounds?
a)
They form hard, brittle crystals with characteristic shapes
b)
They have low melting points
c)
They have low boiling points
d)
They contain no charged particles
44.
In what form can an ionic compound conduct electricity?
a)
when dissolved in water
b)
as a solid
c)
as a crystal
d)
when warmed slightly
45.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
46.
Which of the following describes covalent bonds?
a)
Bonds form because of opposite charges
b)
Bonds form to fill outer electron shells
c)
Electrons are transferred between atoms
d)
Covalent bonds are magical
47.

If an atom has no charge, which of the following must be true?

a)

It has more neutrons than protons or electrons.

b)

There are only neutrons inside the atom.

c)

Its number of protons is equal to its number of electrons.

d)

The neutrons in the atom outnumber the electrons and protons.

48.

Which of these are an ion?

a)

3 protons, 3 neutrons, 3 electrons.

b)

8 protons, 8 neutrons, 8 electrons

c)

2 protons, 3 neutrons, 2 electrons

d)

6 protons, 6 neutrons, 7 electrons

49.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
None
d)
conduct electricity
50.

Which of the compounds below contains a single covalent bond?

a)

A. Br2

b)

B. SO

c)

C. HCl

d)

Both a and c

51.
Which three nonmetals exist only as diatomic molecules?
a)
H, C, Br
b)
N, O, S
c)
I, F,N
d)
H, O, P
52.
A molecule with a double covalent bond is....
a)
HCl
b)
SO
c)
I2
d)
N2
53.
What do we call a covalent bond where electrons are shared UNEVENLY or UNEQUALLY?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
54.

Which is stronger...

a)

N − N

b)

N = N

c)

N ≡ N

55.
Polar, nonpolar, or ionic?
a)
Nonpolar
b)
Polar
c)
Ionic
d)
Pizza
56.
The red numbers in the image below represent ________
a)
subscripts
b)
coefficients
c)
I don't know, and don't want to try
d)
None of the answers are correct
57.
The blue numbers in the image below represent ________
a)
I don't know, and don't want to try
b)
coefficients
c)
subscripts
d)
none of the answers are correct
58.
 H2 + 2O2  -->  2H2O 
a)
Syntheiss
b)
Decomposition
c)
Double Replacement
d)
Single Replacement
59.
A compound reactant splits up to make 2 or more new products.
a)
Syntheiss
b)
Decomposition
c)
Double Replacement
d)
Single Replacement
60.
When two reactant compounds switch partners to make two new products.
a)
Syntheiss
b)
Decomposition
c)
Double Replacement
d)
Single Replacement
61.

CO + ___H2 --> CH4 + H2O

a)

1

b)

2

c)

3

d)

4

62.

4Ag + O2 --> ___Ag2O

a)

1

b)

2

c)

3

d)

4

63.

___AlBr3 + 3Cl2 --> 2AlCl3 + 3Br2

a)

1

b)

2

c)

3

d)

4

64.
In the reaction
2Ca(s) + O2(g) --> 2CaO(s), calcium is __________
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
65.
What is the oxidation number of N in NO2-1?
a)
-3
b)
+4
c)
-2
d)
+3
66.
What is oxidation number of Fe in FeO ?
a)
+2
b)
-2
c)
0
d)
+1
67.
If an atom loses electrons during a chemical reaction, the atom was:
a)
Oxidized
b)
Reduced
c)
Neutralized
d)
Precipitated
68.
Reduction involves 
a)
gaining electrons; gaining oxygen
b)
losing electrons; losing oxygen
c)
gaining electrons, losing oxygen
d)
losing electrons; gaining oxygen
69.
What is the name of Groups 17?
a)
Alkali Metals
b)
Alkali Earth Metals
c)
Transition Metals
d)
Halogens
70.
Where are the metals on the Periodic Table?
a)
To the left
b)
In the upper right hand corner
c)
On the zigzag line
d)
At the bottom
71.
Where are the nonmetals on the Periodic Table?
a)
To the left
b)
In the upper right hand corner
c)
On the zigzag line
d)
At the bottom
72.
How would you describe reactivity on the periodic table?
a)
Elements in the same group are most likely to react.
b)
Elements in the same Periodic are most likely to react.
c)
Elements on opposite sides of the Periodic Table are most likely to react.
d)
There is no trend of reactivity.
73.

Across a period in the periodic table, atomic radii generally

a)

decrease

b)

decrease, then increase.

c)

increase.

d)

increase, then decrease.

74.

Down a group in the periodic table, atomic radii generally

a)

decrease.

b)

remain constant.

c)

increase.

d)

vary unpredictably.

75.

An element with the lowest electronegativity would be found in of the periodic table.

a)

Group 1, Period 7

b)

Group 3, Period 4

c)

Group 5, Period 3

d)

Group 17, Period 2

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