Free Printable AP Chemistry Unit 1: IYKYK

1.

Unit 1: When an electron is in a higher energy level, it is farther away from the nucleus and has less Coulombic attraction to the nucleus and is therefore easier to remove

a)

True

b)

False

2.

Unit 1: When reading a PES graph, the higher the peak, the less electrons there are in that sublevel, and a larger binding energy means that the electrons are closer to the nucleus.

a)

True

b)

False

3.

Unit 1: Isotopes of an element have the same number of protons, but different numbers of electrons.

a)

True

b)

False

4.

Unit 1: Cations (+) are smaller than their atoms since you are removing valence electrons that are farther from the nucleus and anions (−) are larger than their atoms since adding extra electrons increases electron-electron repulsions.

a)

True

b)

False

5.

Unit 1: The greater the electronegativity difference between 2 atoms, the more polar the bond becomes.

a)

True

b)

False

6.

Unit 1: % error= (experimental - theoretical)/experimental

a)

True

b)

False

7.

Unit 1: Filtering separates mixtures based on differences in what property?

a)

Chemical

b)

Solubility

c)

Particle size

d)

Density

8.

Unit 1: What is the equation for calculating the density of a substance?

a)

D=m/v

b)

m=D/v

c)

D=v*m

d)

D=v/m

9.

Unit 1: When an electron is in a lower energy level, it is ________________ away from the nucleus

a)

Closer

b)

Farther

10.

Unit 1: When reading a PES (Photoelectric Spectroscopy) graph, what does the height of a peak represent?

a)

The number of electrons

b)

The number of protons

c)

The mass or the isotope

d)

The amount of energy the electron has

11.

Unit 1: Isotopes of an element have the same number of __________, but different number of __________.

a)

protons, neutrons

b)

neutrons, protons

c)

protons, electrons

d)

electrons, protons

12.

Unit 1: When reading a PES (Photoelectron Spectroscopy) graph, a larger binding energy means that the electrons are _________________ the nucleus?

a)

Closer to

b)

Farther from

13.

Unit 1: Distillation separates mixtures based on differences in what property?

a)

Solubility

b)

Boiling Point

c)

Particle Size

d)

State of Matter

14.

Unit 1: What type of change conserves mass?

a)

none

b)

chemical

c)

physical

d)

chemical and physical

15.

Unit 1: When an electron is in a higher energy level, it has ___________ Coulombic attraction to the nucleus

a)

More

b)

Less

16.

Unit 1: What is the measurement of the burette? (in mL)

a)

6.6mL

b)

6.64mL

c)

7.36mL

d)

7.3mL

17.

Unit 1: Which orbital comes after 4s?

a)

3d

b)

5s

c)

4p

d)

4d

18.

Unit 1: Are cations larger or smaller than their neutral atoms?

a)

Larger

b)

Smaller

c)

Same size

19.

Unit 1: Which piece of glassware is the most precise

a)

beaker

b)

graduated cylinder

c)

burette

d)

test tube

20.

Unit 1: Moving across a row (L to R) on the periodic table, Z_eff _________________

a)

Increases

b)

Decreases

c)

Stays the same

21.

Unit 1: What type of change separates a compound into elements?

a)

physical

b)

chemical

c)

chemical and physical

22.

Unit 1: Why do atoms get smaller moving across a period (L to R) on the periodic table?

a)

More protons (q) to attract the electrons

b)

Fewer protons (q) to attract the electrons

c)

More energy shells (r) so it can't attract the electrons

d)

Fewer energy shells (r) so it attracts the electrons closer

23.

Unit 1: Why are anions larger than their neutral atoms?

a)

More shielding that repels the other electrons

b)

Fewer protons to attract electrons

c)

More electrons to attract protons

d)

More Zeff to attract electrons

24.

Unit 1: Which piece of glassware is the least precise?

a)

graduated cylinder

b)

beaker

c)

burette

25.

Unit 1: When an electron is in a lower energy level, it has a ________________ 1st ionization energy

a)

Higher

b)

Lower

c)

Same

26.

Unit 1: Which electrons are removed first when making a cation?

a)

s

b)

p

c)

d

d)

f

27.

Unit 1: What do mass spectroscopy graphs measure?

a)

Mass of isotopes

b)

Mass of protons

c)

Energy of electrons

d)

Number of electrons

28.

Unit 1: When reading a PES graph, a larger binding energy means that the electrons are ____________ from the nucleus?

a)

closer

b)

farther

c)

the same distance

29.

Unit 1: Which orbital comes after 4p?

a)

5s

b)

4s

c)

3d

d)

4p

30.

Unit 1: germanium is a ________________, hydrogen is a _________________ and uranium is a ________________

a)

metal, non-metal, metalloid

b)

metalloid, non-metal, metal

c)

non-metal, metal, metalloid

31.

Unit 1: Are anions larger or smaller than their neutral atoms?

a)

Larger

b)

Smaller

c)

Same size

32.

Unit 1: When an electron is in a lower energy level, it has a ___________ 1st ionization energy

a)

Higher

b)

Lower

33.

What is the molar mass of Cl₂?

a)

17 g/mol

b)

35.5 g/mo;

c)

71.0 g/mol

d)

89 g/mol

34.

Calculate the molar mass of KOH.

a)

28 g/mol

b)

56 g/mol

c)

84 g/mol

d)

112 g/mol

35.

Calculate the molar mass of Ba(C₂H₃O₂)₂

a)

255.3 g/mol

b)

237.3 g/mol

c)

228.3 g/mol

d)

196.3 g/mol

36.

What is the molar mass of the diatomic element nitrogen?

a)

7 g/mol

b)

14 g/mol

c)

28 g/mol

37.

CO₂

a)

Ionic

b)

Covalent

c)

Polyatomic Ion

d)

Metallic

38.

What two types of atoms make a covalent bond?

a)

2 Nonmetals

b)

1 Nonmetal and 1 Metal

c)

2 Metals

d)

2 Noble Gases

39.

Ionic bonds form between metals and ____.

a)

metalloids

b)

metals

c)

nonmetals

40.

Beryllium and sulfur will form a ______ bond

a)

ionic

b)

covalent

c)

metalloid

41.

MgO

a)

ionic

b)

covalent

c)

metallic

42.

Which concept is Avogadro's number related to?

a)

Mole

b)

Atomic number

c)

Chemical equation

d)

Molar mass

43.

What does Avogadro's number allow scientists to determine?

a)

The temperature of atoms or molecules in a given amount of substance.

b)

The color of atoms or molecules in a given amount of substance.

c)

The weight of atoms or molecules in a given amount of substance.

d)

The number of atoms or molecules in a given amount of substance.

44.

Avogadro's number is approximately equal to:

a)

3.141 x 10^23

b)

9.999 x 10^22

c)

1.234 x 10^24

d)

6.022 x 10^23

45.

How many molecules are in 2.5 mol of NaCl?

a)

1.51x10²³

b)

146

c)

4.15

d)

1.51x10²⁴

46.

How do you solve the following problem: How many grams are there in 7.5 moles of H2SO4?

a)

Convert liters to moles then moles to grams

b)

Convert particles to moles then moles to grams

c)

Convert moles to grams

d)

Convert grams to moles

47.

Match the following...

a)

You convert moles to grams by...

1.

multiplying by the molar mass

b)

You convert liters to moles by...

2.

dividing by 22.4L

c)

You convert moles to particles by...

3.

multiplying my avagadro's constant

d)

You convert grams to moles by...

4.

dividing by the molar mass

e)

You convert moles to liters by...

5.

multiplying by 22.4L

48.

How many grams are in $9.28x10^{23}\ molecules$ of NaCl?

Choose the correct setup.

a)

$9.28x10^{23}\ molecules\ \times\frac{6.02x10^{23}\ grams}{1\ mole}$

b)

$9.28x10^{23}\ molecules\ \times\frac{6.02x10^{23}\ mc}{1\ mole}\times\frac{58.44\ g}{1\ mole}$

c)

$9.28x10^{23}\ molecules\ \times\frac{1\ mole}{6.02x10^{23}\ mc}\times\frac{58.44\ g}{1\ mole}$

d)

$9.28x10^{23}\ molecules\ \times\frac{58.44\ g}{1\ mole}$

49.

How many moles are in 2.67x10²⁴ molecules of H₂O?

What is the missing piece?

$2.67x10^{24}\ molecules\times\frac{???????????}{6.02x10^{23}\ mc}$

a)

6.02x10²³ mc

b)

1 mole

c)

18.016 grams

d)

2.67x10²⁴ mc

50.

What element is this?

a)

Chlorine

b)

Lithium

c)

Boron

d)

Phosphate

e)

Phosphite

51.

If you had 192.9 atoms of silver, 100 would be Ag-107 and 92.9 would be Ag-109. What would the Average Atomic Mass be? (You have time to answer... do your work...)

Important numbers: Atomic Mass of Ag-107 is 106.905 and Atomic Mass of Ag-109 is 108.904.

a)

107.87

b)

108.85

c)

107.44

d)

108.26

e)

107.94

52.

What are isotopes?

a)

charged atoms

b)

radioactive elements

c)

elements with different numbers of neutrons

53.

What are the steps of operation in the mass spectrometer?

a)

Accelerate, Deflect,Ionize, Detect

b)

Deflect,Ionize, Accelerate, Detect

c)

Ionize, Accelerate, Deflect, Detect

d)

Detect, Accelerate, Deflect, Ionize

54.

What do the peaks on the mass spectrum represent?

a)

anions

b)

different isotopes

c)

atoms with differing numbers of electrons

d)

numbers of electrons

55.

Which element does this mass spectrum most likely represent?

a)

neon

b)

scandium

c)

boron

d)

sodium

56.

What do the heights of the peaks represent in the mass spectrum?

a)

number of isotopes

b)

relative abundance of each isotope

c)

average atomic mass

d)

charge:mass ratio

57.

How many isotopes are shown in this mass spectrum?

a)

1

b)

84

c)

86

d)

4

58.

Based on the mass spectrum, which isotope of chlorine is most abundant?

a)

³⁵Cl

b)

³⁷Cl

c)

⁷⁰Cl

d)

⁷²Cl

59.

Carbon has three known isotopes. Which is the most abundant?

a)

carbon-12.011

b)

carbon-12

c)

carbon-13

d)

carbon-14

60.

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

61.

Molecular Formula = C₂F₆

Choose the correct empirical formula.

a)

CF

b)

C₂F₆

c)

C₃F

d)

CF₃

62.

Empirical Formula = CF₂

Molecular formula mass = 192 g/mol

Molecular Formula = ?

a)

C₄F₈

b)

C₈F₄

c)

C₃F₆

d)

C₂F₄

63.

What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?

a)

C3H8

b)

CH4

c)

C2H2

d)

C4H10

64.

What percentage of the total atomic mass of carbon monoxide (CO) is composed of carbon?

a)

29%

b)

43%

c)

57%

d)

73%

65.

What percentage of the total atomic mass of carbon monoxide (CO) is composed of oxygen?

a)

29%

b)

43%

c)

57%

d)

73%

66.

which one defines percent composition?

a)

the percent by mass of each element in a compound

b)

when elements join together

c)

when water dries up

d)

elements split

67.

How do you calculate the percent composition by mass of an element in a compound?

( (a) ) $\div$ ( (b) ) $\times$ 100

Choose from the below words

Total Molar Mass of Element in Compound

Total Molar Mass of Compound

Molar Mass of a Single Element

100

68.

% to Mass; Mass to Moles; Divide by Small; Multiply Till Whole

a)

Steps to find an Empirical Formula

b)

Steps to find a Molecular Formula

c)

Steps to find % Composition

69.

Weight of the Molecular Formula Divided by the Weight of the Empirical Formula x 100

a)

Steps to find an Empirical Formula

b)

Steps to find a Molecular Formula

c)

Steps to find Percent Composition

70.

Individual divided by total x 100

a)

Steps to find an Empirical Formula

b)

Steps to find a Molecular Formula

c)

Steps to find Percent Composition

71.

Click the hotspot for the box that represents an element.

A

B

C

D

72.

Click the hotspot that represents a mixture

A

B

C

D

73.

Identify the substance in box Y.

a)

element

b)

compound

c)

mixture

74.

Identify this substance.

a)

element

b)

compound

c)

mixture

75.

Identify this substance.

a)

element

b)

compound

c)

mixture

76.

Which electron configuration belongs to Chlorine (Cl)?

a)

1s²2s²2p⁶3s²3p⁵

b)

1s²2s²2p⁶3s²3p⁶

c)

1s²2s²2p⁶3s²3p⁷

77.

What atom matches this electron configuration?
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰

a)

Zinc (Zn)

b)

Copper (Cu)

c)

Nickel (Ni)

d)

Germanium (Ge)

78.

The PES spectrum below is for the element _______________.

a)

O

b)

Ne

c)

N

d)

F

79.

Examine the spectrum below. Where would you expect the 2p peak for F be if it were on the same spectrum?

a)

To the left of the peak at 3.04

b)

To the right of the peak at 3.04

c)

To the left of the peak at 1.31

d)

To the right of the peak at 1.31

80.

What does the 4th peak from the left represent?

a)

The 2s electrons

b)

The 3d electrons

c)

The 2p electrons

d)

The 3s electrons

81.

Which electrons would be ejected with the most kinetic energy according to the spectrum below?

a)

The ones in the peak at 151

b)

The ones in the peak at 7.9

c)

The ones in the peak at 1.09

d)

The ones in the peak at 0.58

82.

Which peak (or peaks) correspond to the valence electrons?

a)

The peak at 1

b)

The peaks at 1 and 2.05

c)

The peak at 239

d)

The peaks at 239 and 22.7

83.

How many valence electrons does the element pictured in the PES spectrum below have?

a)

1

b)

2

c)

3

d)

4

84.

As the energy level goes higher, the electrons

a)

have lower in energy

b)

are more stable

c)

are weaker

d)

are farther from the nucleus

85.

Click on the hotspot that represents an energy level.

A

B

C

D

E

F

86.

The lowest available energy state of an electron is called the:

a)

the lowest state

b)

the ground state

c)

the entry state

d)

the fixed state

87.

What is the label for energy?

a)

J

b)

m

c)

Hz

d)

nm

88.

Valence electrons are found in the ______ energy level.

a)

Farthest in

b)

Middle

c)

Outermost

89.

Select the hotspot that shows the most EN element

A

B

C

D

E

F

90.

Select the hotspot that shows the smallest element

A

B

C

D

E

F

91.

Select the hotspot that shows the largest element

A

B

C

D

E

F

92.

Select the hotspot that shows the largest 1st ionization energy

A

B

C

D

E

93.

Reorder the following in order of increasing atomic radius

a)

F

b)

Cl

c)

Br

d)

I

e)

At

1)

2)

3)

4)

5)

94.

Reorder the following in order of increasing atomic radius.

a)

Cl

b)

S

c)

P

d)

Si

e)

Al

1)

2)

3)

4)

5)

95.

Reorder the following in order of increasing EN

a)

Ni

b)

Cu

c)

N

d)

O

e)

F

1)

2)

3)

4)

5)

AP Chemistry Unit 1: IYKYK

Total questions: 95

Worksheet time: 2hrs 41mins

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