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Chem A CP Tri 2 Unit 4 Review

Total questions: 60

Worksheet time: 53mins

Name
Class
Date
1.

The ability of an atom in a molecule to attract electrons is...

a)

electromagnetism

b)

ionization energy

c)

electronegativity

d)

first ionization energy

2.

How many moles are in 24g of Sulfur (S)? (1 mole S = 32.065g S)

a)

4.6g

b)

0.75

c)

7.7 x 1027.7\ x\ 10^2  

d)

7.9

3.

A solution has a density of 1.22g/mL. What is the mass of the solution with a volume of 4.35mL?

a)

5.31g

b)

39.5g

c)

1.22g

d)

3.57g

4.

931g is the same as

a)

.931kg

b)

9.31mg

c)

93,100cg

d)

93.1 dg

5.

How many hours are in 24.95 minutes?

a)

4,158

b)

0.42

c)

0.4158

d)

4,200

6.

What type of decay does this symbol represent?

a)

beta decay

b)

alpha decay

c)

gamma decay

d)

fusion

7.

This orbital diagram represents:

a)

Carbon

b)

Boron

c)

Nitrogen

d)

Oxygen

8.

Electronegativity (a)   as you go down a group.

9.

Which element has a lower electronegativity value?

a)

Calcium

b)

Barium

10.
Compounds are different than elements because compounds are -
a)
A combination of two or more elements.
b)

B)not able to be broken down into parts
c)
made from the same type of atoms
d)
a pure substance, elements are not
11.
What is the difference between a compound and an element?
a)

Compounds are made up of elements and can be chemically separated. Elements cannot be separated.

b)

Elements make up compounds. Elements can be separated but compounds cannot be separated.

c)

Elements are found on the periodic table and compounds are found on the dining room table.

12.

How well measurements agree with the "real value" is called ............

a)

accuracy

b)

precision

c)

calcuation

13.

The degree of exactness of measurement is called ...........

a)

acuuracy

b)

precision

c)

calculation

14.

What is the correct scientific notation for 4,576,000?

a)

5×1065\times10^6  

b)

4,576,000

c)

4,576×1034,576\times10^3  

d)

5.476×1065.476\times10^6  

15.

9001.6−200=9001.6-200=  

a)

9,000

b)

8,801.6

c)

8,800

d)

8,802

16.

302.000×47=302.000\times47=  

a)

14,194

b)

14,000

c)

15,000

d)

14,194.000

17.

62+0.98=62+0.98=  

a)

62

b)

62.98

c)

63.0

d)

63

18.

What subatomic particles are in the nucleus?

a)

Protons

b)

Neutrons

c)

Electrons

d)

Photons

19.

An isotope has three forms.  10% have a mass of 4 amu, 20% have a mass of 5 amu and 70% have a mass of 6 amu.  

Based on the percentage of abundances above, the average atomic mass will be closest to...

a)

3 amu

b)

4 amu

c)

5 amu

d)

6 amu

e)

None of the above

20.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
5
21.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
22.

Titanium is in group 4. What period is it in?

a)

2

b)

3

c)

4

d)

5

23.

What two elements are most similar in their chemical properties?

a)

Na and Br

b)

C and Ge

c)

Cs and Ba

d)

I and Xe

24.
The parts of a homogeneous mixture are   __________ throughout. 
a)
Same 
b)
Different 
c)
Neutral 
d)
Suspended 
25.
___________ is a combination of substances that can be physically separated. 
a)
Colloid 
b)
Mixture 
c)
Suspension 
d)
Compound 
26.

Sugar and water

a)

Homogeneous

b)

Heterogeneous

27.

Oil and water

a)

Homogeneous

b)

Heterogeneous

28.

6. Chicken noodle soup is an example of

a)

Heterogeneous mixture

b)

Homogeneous mixture

29.

Chlorine forms an ion with a charge of ...

a)

2+

b)

1+

c)

1-

d)

3-

30.

Magnesium forms an ion with a charge of ...

a)

1+

b)

1-

c)

3+

d)

2+

31.
What is 50 C in Kelvin?
a)
223
b)
323
c)
100
d)
50
32.
Which example best describes a physical change?
a)
iron rusting
b)
charcoal burning
c)
an ice cube melting
d)
a marshmallow burning
33.
Sodium Hydroxide dissolves in water
a)
Chemical Change
b)
Physical Change
34.
Hydrochloric acid reacts with potassium hydroxide to produce a salt, water,and heat.
a)
Chemical Change
b)
Physical Change
35.

The frequency of light is 7.14 x 1014 Hz. What is the wavelength?

a)

3.00 x 108 m

b)

4.20 x 10-7 m

c)

2.25 x 1023 m

d)

3.90 x 10-9 m

36.

When bombarded with light, lithium emits a light with a frequency of 4.29 x 1014 Hz. Calculate the wavelength and use the chart to predict the color.

a)

blue

b)

green

c)

yellow

d)

red

37.

Calculate the energy of light with a frequency of 5.10 x 1014 Hz.

a)

3.38 x 10-19 J

b)

5.88 x 10-7 J

c)

9.62 x 1012 J

d)

1.04 x 10-13 J

38.
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
39.

Which of the following is a compound?

a)

Titanium in a golf club

b)

Aluminum in a can

c)

Mercury in a thermometer

d)

Salt (NaCl) in a shaker

40.

Which has the smallest atomic radius?

a)

Li

b)

Br

c)

Xe

d)

Rb

41.

The identity of an element can be determined by...

a)

# of electrons

b)

Mass number

c)

# of protons

d)

Average atomic mass

42.

The sublevel that can hold a maximum of 14 electrons is...

a)

s

b)

p

c)

f

d)

d

43.

The _____ the element is in determines the number of valence electrons it has.

a)

period/row

b)

group/column

44.

Valence electrons are the

a)

outer most electrons in an atom

b)

total electrons in an atom

45.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
46.
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
47.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
48.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
49.

Which particle is responsible for bonding?

a)

Protons

b)

Electrons

c)

Neutrons

d)

Nucleus

50.
A wave with a large wavelength will have a ______ frequency and _____ energy
a)
high, low
b)
high, high
c)
low, high
d)
low, low
51.
Select the correct order of waves on the EMS 
a)
Radio, Micro, Infra, Visible, Ultra, X-ray, Gamma
b)
Gamma, X-ray, Ultra, Vis, Infra, Micro, Radio
c)
Vis, Micro, Infra, Ultra, X-ray, Gamma, Radio
d)
Micro, Radio, Vis, Infra, Ultra, X-ray, Gamma
52.
Which has the LONGEST wavelength and, therefore, the lowest frequency/energy
a)
Gamma Rays
b)
Radio Waves
c)
Visible Light
d)
Infrared rays
53.

Which of the following has the shortest wavelength?

a)

microwaves

b)

UV rays

c)

Infrared

d)

the color blue

54.
High frequency waves have _________ wavelengths.
a)
varying
b)
long
c)
the same
d)
short
55.

How many neutrons are there in 226Ra?

a)

88

b)

138

c)

226

d)

314

56.

What is the lowest possible energy level that an electron can occupy?

a)

Excited state

b)

Fundamental state

c)

Ground state

d)

Outermost state

57.

The figure shows different possible transitions of electrons as they move from higher energy states to lower energy states. Which transition will produce the spectrum line with the lowest wavelength in this element’s atomic spectrum?

a)

A

b)

B

c)

C

d)

D

58.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
59.

Which shape represents the shape of an "s" orbital?

a)
b)
c)
d)
60.

Which shape represents the shape of an "p" orbital?

a)
b)
c)
d)

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