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Semester 1 Exam Review

Total questions: 46

Worksheet time: 2hrs 36mins

Name
Class
Date
1.

You should only touch the lab equipment

a)

after you enter the lab

b)

before you enter the lab

c)

after you have be instructed to

d)

when you get home

2.

Appropriate dress includes

a)

flip flops

b)

closed toed shoes

c)

snow shoes

d)

flippers

3.

You should never ______ chemicals in the lab without your teachers permission.

a)

taste

b)

touch

c)

smell

d)

all of the above

4.

The white square on the hazmat symbol represents

a)

health hazards

b)

flammability

c)

reactivity

d)

Other considerations

5.
How many sig figs are there?
100.00
a)
1
b)
3
c)
4
d)
5
6.
How many sig figs are there?
4004
a)
1
b)
2
c)
3
d)
4
7.
How many sig figs are there?
0.000008
a)
1
b)
2
c)
6
d)
7
8.
How many sig figs are there?
0.00400
a)
1
b)
3
c)
5
d)
6
9.

Solve. Round using SigFig math rules.

12.5 mL + 20.05 mL + 2.69 mL

a)

35 mL

b)

35.2 mL

c)

35.24 mL

d)

35.240 mL

10.

Solve. Round using SigFig math rules.

103 cm x 11 cm

a)

11 cm2

b)

1100 cm2

c)

1130 cm2

d)

1133 cm2

11.

Solve. Round using SigFig math rules.

1.3562 mL / 14.32 g

a)

0.094 mL/g

b)

0.0947 mL/g

c)

0.094706 mL/g

d)

0.09471 mL/g

12.
What tool is used to measure liquid volume?
a)
meter stick
b)
triple beam balance
c)
LxWxH
d)
Graduated Cylinder
13.
What is the metric unit for temperature?
a)
Kelvin
b)
Celsius
c)
Farenheit
d)
Absolute zero
14.
Find the volume of the liquid.
a)
39 mL
b)
38 mL
c)
30.8 mL
d)
38 cm3
15.
A meter is equal to how many centimeters?
a)
1000
b)
100
c)
10
d)
1
16.
Convert 3.75 kg to grams. 
a)
3750 g 
b)
375 g
c)
37.5 g
d)
3.750 g
17.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
18.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
19.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
20.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
21.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
22.

Which of these combinations is an ionic compound made of?

a)

Metal and Metal

b)

Nonmetal and Nonmetal

c)

Metal and Nonmetal

d)

Cation and Cation

23.

Whose model suggested that negative particles were mixed in with positively charged material - like seeds in a watermelon?

a)

J.J. Thomson

b)

Ernest Rutherford

c)

Niels Bohr

d)

Albert Einstein

24.

Who discovered that the atom had an small, dense, positively charged center?

a)

Ernest Rutherford

b)

J.J Thomson

c)

Robert Millikan

d)

John Dalton

25.

Who named the positive center of the atom the "nucleus?"

a)

Democritus

b)

Dalton

c)

Thomson

d)

Rutherford

26.

Who proposed that electrons move around the nucleus in circular orbits?

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

27.

What law states that, regardless of the amount, a compound is always composed of the same elements in the same proportion by mass?

a)

Law of definite proportions

b)

Law of conservation of mass

c)

Law of multiple proportions

d)

Law of mass action

28.
Convert 8 kilometers to meters
a)
800 m
b)
80,000 m
c)
8,000 m
d)
.008 m
29.
Is 20 g greater than, less than, or equal to 2 kg?
a)
greater than
b)
less than
c)
equal to
30.
There are ___ millimeters in 7.3 centimeters
a)
730
b)
.73
c)
73
d)
.073
31.
750 g is ____________  .75 kg?
a)
greater than
b)
less than
c)
equal to
d)
not the same as
32.
240 cm = ___________ m
a)
2400
b)
24
c)
2.4
d)
0.24
33.
3 km = ___________ mm
a)
30
b)
300
c)
3,000
d)
3,000,000
34.
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
35.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
36.
List the following in order of weakest to strongest ionization energy.
P, Cs, Co, Sr
a)
P, Co, Sr, Cs
b)
Cs, Sr, Co, P
c)
Sr, Cs, Co, P
d)
P, Co, Cs, Sr
37.

Which of the following elements has the smallest atomic radius?

a)

Sulfur

b)

Chlorine

c)

Aluminum

d)

Sodium

38.

Which of the following will have a lower ionization energy than Scandium (Sc)?

a)

Helium (He)

b)

Titanium (Ti)

c)

Calcium (Ca)

d)

Magnesium (Mg)

39.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
40.
Atomic radius generally increases as we move __________.  
a)
down a group and from right to left across a period 
b)
up a group and from left to right 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 
41.
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
42.

The electronegativity of Cl is the highest in Period 3. Why?

a)

Cl is the largest and has the greatest effective nuclear charge

b)

Cl is the smallest and has the lowest effective nuclear charge

c)

Cl is the largest and has the lowest effective nuclear charge

d)

Cl is the smallest and has the greatest effective nuclear charge

43.
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.
44.

The element with the lowest electronegativity in Period 3 is

a)

Na

b)

Cl

c)

Ar

d)

Mg

45.

Why does ionization energy decrease going down a group?

a)

Adding more energy levels moves the valence e- further from the nucleus

b)

There are more valence electrons in the outer shell

c)

There are more protons in the nucleus

d)

There are less protons in the nucleus

46.

Metals form

a)

positive anions

b)

negative anions

c)

positive cations

d)

negative cations

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