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Worksheets

Quarter 1 Final

Total questions: 85

Worksheet time: 1hrs 21mins

Name
Class
Date
1.
You should never ______ chemicals in the lab. 
a)
taste
b)
touch
c)
smell
d)
all of the above
2.

Approved eye protection (such as goggles) are worn in the laboratory...

a)

to avoid eye squinting.

b)

to improve your vision.

c)

only if you do not have glasses.

d)

any time chemicals, heat, or glassware are used.

3.

After completing an experiment, all chemical wastes should be...

a)

left at your lab station for the next class.

b)

disposed of according to your teacher's directions.

c)

dumped in the sink.

d)

taken home.

4.

Before you leave the science room, you should...

a)

clean your work area and equipment.

b)

return all equipment to the proper storage area.

c)

wash your hands with soap and water.

d)

all of the above.

5.

True of False: All chemicals in the lab, including food and store-bought chemicals, should be treated as if they could be hazardous.

a)

True

b)

False

6.

What is this piece of lab equipment?

a)

beaker

b)

flask

c)

graduated cylinder

d)

test tube

7.

What is this piece of lab equipment?

a)

hot plate

b)

flame thrower

c)

heater

d)

bunsen burner

8.

What is this piece of lab equipment?

a)

buret

b)

erlenmeyer flask

c)

graduated cylinder

d)

beaker

9.
Identify the equipment shown here:
a)
beaker
b)
Erlenmeyer flask
c)
Florence flask
d)
volumetric flask
10.
Identify the equipment shown here:
a)
striker
b)
test tube holder
c)
flame snuffer
d)
utility clamp
11.

How would you write 564,000,000 in scientific notation?

a)

564 x 10-6

b)

564 x 106

c)

5.64 x 108

d)

56.4 x 107

e)

5.64 x 10-8

12.
Which of the following is correct scientific notation?
a)
20.35 x 104
b)
.2035 x 104
c)
2035 4
d)
2.035 x104
13.

When converting a number written in scientific notation to long form, If the exponent is a negative number...

a)

you will get a large number

b)

you will get a small number

14.

How do you write

8.317 x 106

in long form?

a)

8, 371, 000, 000

b)

000 000. 831 7

c)

.000 008 317

d)

8, 317, 000

15.

Solve the following equation for r:

C = Prt

a)

r = CPtr\ =\ \frac{C}{Pt}

b)

r=PtCr=\frac{Pt}{C}

c)

r=C−Ptr=C-Pt

d)

r = CPtr\ =\ CPt

16.

Solve the following equation for A

 L =AWL\ =\frac{A}{W}  

a)

 A=L×WA=L\times W  

b)

 A = LWA\ =\ \frac{L}{W}  

c)

 A = WLA\ =\ \frac{W}{L}  

d)

 A = L − WA\ =\ L\ -\ W  

17.

Solve this equation for x

 z = kxz\ =\ \frac{k}{x}  

a)

 x=zkx=\frac{z}{k}  

b)

 x=kzx=\frac{k}{z}  

c)

 x = kzx\ =\ kz  

d)

 x = k−zx\ =\ k-z  

18.

Using the equivalents below determine how many tolls are in 398 smacks.

4 tolls = 9 smacks

a)

177 tolls

b)

896 tolls

c)

3,582 tolls

d)

1,592 tolls

e)

14,328 tolls

19.

Using the equivalents below, determine how many smacks are in 25 largos.

4 tolls = 9 smacks ; 12 tolls = 5 largos

a)

135 smacks

b)

23.5 smacks

c)

60 smacks

d)

54, 000 smacks

e)

37 smacks

20.

Using the equivalents below, determine how many doodles are in 25 largos.

8 largos = 7 fleas; 2 fleas = 5 doodles

a)

54.7 doodles

b)

71.4 doodles

c)

8.75 doodles

d)

11.4 doodles

e)

21.88 doodles

21.

What type of mixture is this? (Trail Mix)

a)

Homogenous mixture

b)

Compound

c)

Heterogeneous mixture

d)

Element

22.

Kool-Aid is an example of a(n)

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

23.

Mercury (Hg) is an example of a(n)

a)

Element

b)

Compound

c)

Homogeneous mixture

d)

Heterogeneous mixture

24.

Baking Soda (NaHCO3) is an example of what?

a)

Element

b)

Compound

c)

Heterogeneous mixture

d)

Homogeneous mixture

25.

Identify the particles (tightly compact and organized)

a)

solid

b)

liquid

c)

gas

d)

none

26.
What happens to particles when they are heated?
a)
They speed up and spread out
b)
They slow down and compress
c)
They stop moving
d)
They move closer together and speed up
27.

Breaking a window is an example of

a)

Physical Change

b)

Chemical Change

28.
Which of the following is NOT an example of a physical change?
a)
crumpled paper
b)
pencil sharpening
c)
shrunken clothing
d)
sour milk
29.

Chemical or Physical:

The words "blue", "large", and "soft" all describe __________ properties.

a)

Chemical

b)

Physical

30.

Chemical or Physical:

The ability to burn is a _______________ property of wood, but not a property of silver.

a)

Chemical

b)

Physical

31.

Look at this image. Which object has the LOWEST density? How?

a)

The Ping Pong Ball because it floats to the top

b)

The bolt because it has sunk to the bottom

c)

The soda cap because it is not just full of air like the Ping Pong ball

32.

Using the picture, tell me which object is the least dense and why?

a)

The fish because he is in the middle

b)

The cork because it is floating at the top of the water

c)

The rock because it is at the bottom

d)

The cork and the rock because they have the same about of atoms.

33.

What is the unit for mass?

a)

Grams (g)

b)

Milliliters (mL)

c)

Grams/Milliliter (g/mL)

34.

What is the unit for Density?

a)

Grams (g)

b)

Milliliters (mL)

c)

Grams/Milliliter (g/mL)

35.

When you put an object in a graduated cylinder of water and measure how much the water level changed what is this process called?

a)

Relative Density

b)

Displacement

c)

Density

36.
What is the volume of Object X?
a)
10.0 cm3
b)
15.0 cm3
c)
20.0 cm3
d)
25.0 cm3
37.
An irregularly shaped piece of gold was lowered into a graduated cylinder holding a volume of water equal to 17 ml. The height of the water rose to 20 ml. If the mass of the gold was 27 g, what was its density?
a)
9 g/mL
b)
10.5 g/mL
c)
6.5 g/mL
d)
8 g/mL
38.
Put the liquids in order from most dense to least dense?
a)
4, 3, 2, 1
b)
1, 2, 3, 4
c)
3, 4, 2, 1, 
d)
4, 3, 1, 2
39.

If the volume is 5 mL and the mass is 25g, what is the density?

a)

5

b)

25

c)

100

d)

50

40.

What is the density? If the mass is 40g and the Volume is 20 mL

a)

2

b)

800

c)

60

d)

20

41.

Most of the mass of an atom is due to:

a)

protons

b)

neutrons

c)

protons + neutrons

d)

electrons

42.

Electrons are found

a)

in the nucleus

b)

outside the nucleus

c)

both in and outside the nucleus

43.

What is the element with the atomic number 12?

a)

sodium

b)

iron

c)

bromine

d)

magnesium

44.

What is the number of electrons in an atom of neon?

a)

10

b)

7

c)

23

d)

100

45.

What is the element with 1 electron?

a)

helium

b)

hydrogen

c)

chlorine

d)

gold

46.

If X is the symbol for an element, which of the following is an isotope of 60132X_{60}^{132}X  

a)


 60130X_{60}^{130}X  

b)

 60132X_{60}^{132}X  

c)

 62130X_{62}^{130}X  

d)

 62132X_{62}^{132}X  

47.

Atoms of the same element have the same

a)

Number of protons

b)

Number of neutrons

c)

Mass number

d)

Mass

48.

An atom of an element with the atomic number 48 and mass number 122 contains:

a)

48 protons, 48 electrons, 74 neutrons

b)

74 protons, 48 electrons, 48 neutrons

c)

120 protons, 48 electrons, and 72 neutrons

d)

72 protons, 72 electrons, and 48 neutrons

49.

What is different about carbon-12 and Carbon-13

a)

Carbon-12 has one less neutron

b)

Carbon-12 has 12 neutrons

c)

Carbon-12 has 24 neutrons

d)

Carbon-12 has no protons

50.

The number in the name iodine-131

a)

The atomic number

b)

The mass number

c)

The sum of protons and electrons

d)

None of these

51.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
52.

What is the maximum number of electrons that an S orbital can have?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

53.

How many electrons can the d orbital hold?

a)

8

b)

10

c)

2

d)

4

54.
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
55.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6
56.

What is incorrect about this orbital diagram?

a)

Both arrows in the 1st 2p orbital should be pointing up

b)

There is nothing incorrect with this diagram

c)

In the 2p energy level, each of the arrow should be in separate orbital, with each pointing upwards.

d)

All the arrows should be pointing up.

57.

The electron-configuration notation for sodium (Na) is 1s2 2s2 2p6 3s1. Which of these options is the correct orbital notation for Sodium?

a)
b)
c)
d)
58.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
59.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
60.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
61.

Valence Electrons of Magnesium

a)

1

b)

2

c)

3

d)

4

62.

All atoms are most stable with (or would "prefer") how many electrons in their valence shell?

a)

1

b)

2

c)

8

d)

18

63.
a)
2
b)
3
c)
5
64.

USE THE PERIODIC TABLE

How many valence electrons does Phosphorus have?

a)

31

b)

5

c)

15

d)

4

65.
Which group has the greatest number of valence electrons?
a)
1
b)
14
c)
18
d)
16
66.
How many valence electrons are found in atoms of group 14?
a)
4
b)
3
c)
14
d)
16
67.

How many valence electrons does this atom have 1s22s22p6

a)

6

b)

5

c)

8

d)

10

68.

How many valence electrons does this atom have?

1s2 2s2 2p6 3s2

a)

8

b)

3

c)

2

d)

12

69.

Which atom has the largest atomic radius?

a)

potassium

b)

rubidium

c)

francium

d)

cesium

70.
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
71.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
72.
Order the following in increasing atomic radii: 
Ra, Be, Ca, Rb, H
a)
Ra, Be, Rb, H, Ca
b)
Rb, H, Ca, Be, Ra
c)
Ra, Rb, Ca, Be, H
d)
H, Be, Ca, Rb, Ra
73.
Which of the following sequences corresponds to a correct trend in ionization energy?
a)
Cl > S > P > Al
b)
Sr > Ca > Mg > Be
c)
Rb > K > Na > Li
d)
Rb > Sr > I > Xe
74.
Which of the following is true about a sulfur atom and a chlorine atom?
a)
Sulfur is larger and has higher ionization energy.
b)
Sulfur is larger and has lower ionization energy.
c)
Sulfur is smaller and has higher ionization energy.
d)
Sulfur is smaller and has lower ionization energy.
75.
Choose the set that goes from lowest to highest electronegativity?
a)
Cu, Mg, Sr, Ca
b)
F, Cl, Br, Si
c)
Cs, Rb, Ca, Mg
d)
Zn, Cd, Ag, Cu
76.
Elements closer to the noble gases have stronger attraction for electrons.
a)
True
b)
False
77.
Which of the following is the least electronegative element?
a)
oxygen
b)
potassium
c)
fluorine
d)
nitrogen
78.

Which group is referred to as Alkali Metals?

a)

3

b)

1

c)

7

d)

17

79.

What is the name of group number 2?

a)

transition metals

b)

halogens

c)

metaloids

d)

alkaline earth metals

80.

A grouping of elements based on similar chemical properties, arranged by columns in the periodic table; also known as a group

a)

family

b)

period

c)

row

d)

isotope

81.

How many electrons would a Nitrogen ion gain/lose?

a)

lose 5

b)

gain 5

c)

lose 3

d)

gain 3

82.

How many electrons would a Calcium ion gain/lose?

a)

lose 1

b)

gain 1

c)

lose 2

d)

gain 2

83.

What is the ion formed from Sulfur?

a)

S+2

b)

S-2

c)

S+6

d)

S-6

84.

A Bromine ion gains 1 electron, which of the following is the correct symbol for a Bromine ion?

a)

Br-1

b)

Br+1

c)

Br+7

d)

Br-7

85.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2

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