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Intro to Chemistry > Final Exam > Flashcards

Final Exam Flashcards

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1
Q

Is Nitrogen
Element, Compound, Heterogeneous or Homogeneous?

A

Element

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2
Q

Is Helium
Element, Compound, Heterogeneous or Homogeneous?

A

Element

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3
Q

Is Coffee
Element, Compound, Heterogeneous or Homogeneous?

A

Homogeneous mixture

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4
Q

Is Mercury
Element, Compound, Heterogeneous or Homogeneous?

A

Element

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5
Q

Is Fruit Salad
Element, Compound, Heterogeneous or Homogeneous?

A

Heterogeneous Mixture

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6
Q

What substances are these?

A

Homogeneous mixtures

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7
Q

What substances are these?

A

Heterogeneous mixtures

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8
Q

Which is a compound and which is a mixture?

A
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9
Q

Identify whether each of the following statements describes Chemical or Physical changes or properties.

1) Sodium chloride is stable and unreactive.
2) The boiling point of hydrogen is 20 K.
3) Nitrogen exists as a gas a room temperature.
4) Sulfer has an unpleasant odor.
5) Chlorine gas is corrosive.
6) Copper conducts electricity.

A

1) Chemical
2) Physical
3) Physical
4) Physical
5) Chemical
6) Physical

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10
Q

Which are these?

A
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11
Q

Which are these?

A
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12
Q

The newly discovered element Nh (Nihonium), with atomic number 113, would be a member of which family:
none of these
the Group 3A elements
the noble gases
the halogens
the transition elements

A

the Group 3A elements

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13
Q

Formaldehyde is a disinfectant, a preservative, and a raw material for plastics manufacture. Its melting point is -92 degrees C and its boiling point is -19.5 degrees C.

Is formaldehyde a gas, liquid, or solid at room temperature (25 degrees C)?

A

gas

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14
Q

Bloods, Honey, wine, water, acetone, Mercury are all what?

A

Liquids

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15
Q

Brick, iron bar, coin, sand, glass, aluminum foil are all what?

A

Solids

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16
Q

Air, Natural gas, Hydrogen, Carbon dioxide, nitrogen, argon are all what?

A

Gases

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17
Q

Which color of visible light has the most energy per photon?

A

Purple

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18
Q

Argon:
Atomic Symbol
Mass
Protons = atomic number
Neutrons = mass number - atomic number
Electrons = atomic number

A

Ar
38
18
20
18

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19
Q

Iodine:
Atomic Symbol
Mass
Protons = atomic number
Neutrons = mass number - atomic number
Electrons = atomic number

A

I
131
53
78
53

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20
Q

Phosphorus:
Atomic Symbol
Mass
Protons = atomic number
Neutrons = mass number - atomic number
Electrons = atomic number

A

P
31
15
16
15

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21
Q

Cadmium:
Atomic Symbol
Mass
Protons = atomic number
Neutrons = mass number - atomic number
Electrons = atomic number

A

116^48Cd
116
48
68
48

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22
Q

How do you find the neutrons of an element?

A

Subtract the atomic number from the atomic mass.

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23
Q

Use the periodic table to determine which one of the following isotopes for each element is the most abundant.

A

Cl-35

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24
Q

Write the number as a whole number or decimal: 8.81 x 10^-3

A

0.00881

move the point 3 to the left because its negative

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25
Q

Write the number in scientific notation:
7,690,000

A

7.69 * 10^6

move the point all the way to the end

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26
Q

Perform the following calculation, expressing the result with the correct number of significant figures. You must have the correct answer and the sig figs correct for credit.
0.564 + 0.0307 =

A

0.595

its always the first number of sig figs, round up

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27
Q

Add the following and express your answer in appropriate scientific notation:
(7.7 x 10^4) + (7.4 x 10^1)

A

7.7074 ×10^4

7.7 x 10^4

only need the 2 numbers of sig figs

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28
Q

Identify whether each of the following substances will Sink or Float in alcohol (0.7860 g/mL).
Ice (0.917)
Hexane (0.659)
Lard (0.82)
Milk (1.03)

remember to make the scale

A

Sink
Float
Sink
Sink

whatever is higher than 0.7860 will sink and under will float

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29
Q

Suppose you were given a piece of unknown metal, with a mass of 23.430 g, and a 50-mL graduated cylinder. You place some water in the cylinder and read that it is 36.0 mL of water.

When you place the metal into the water, the volume rises to 44.1 mL. What is the density of the metal?

A

Find change in water
44.1-36.0=8
Divide that change to the mass of unknown metal
8 / mass 23.430 =
2.9

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30
Q

Heat is best defined as _________.

A

energy transferred as the result of a temperature difference.

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31
Q

The kinetic energy associated with the random motion of molecules is called _________.

A

thermal energy.

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32
Q

The maximum speed a chicken can run is 9.3 miles per hour. How fast is this in meters per second?

A

9.3 * 1609.34 meters / 3600 seconds
= 4.16 meters per second
=4.2

1 mile = 1609.34 meters (exact conversion factor)
1 hour = 3600 seconds

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33
Q

A typical engagement ring might have a diamond made of pure carbon, weighing 0.17 grams.

How many moles of carbon are in that diamond?

How many carbon atoms are in the diamond?

A

molar mass of carbon 12.01
0.17 / 12.01= 0.014

0.01416 mol x 6.022 x 10^23 = 8.5 x 10^21

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34
Q

If a person has a blood glucose level of 109 mg / 100. mL, a level that can cause brain damage, what is the total mass (in grams) of glucose in 4.91 L of blood?

A

109 / 100 = 1.09
1.09 x 4.91 = 5.3519
=5.36

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35
Q

Calculate the molar mass of Mg3(PO4)2. Then calculate the mass percent of Mg in the compound.
molar mass of Mg3(PO4)2:

A

Find the Molar mass for
Mg=24.30, O=15.99, P=30.97
24.30 x 3 + (30.97 + 15.99 x 4) x 2 = 262.86g/mol
(24.30 x 3 / 262.86) x 100
(72.90/262.86) x 100
=27.73%

Mass% of magnesium in compound=(Total mass of Mg/total molar mass)*100

36
Q

A cup of tea contains 54.9 mg of caffeine (C8H10N4O2). What is the molar mass of caffeine?
How many moles of caffeine are present in this cup of tea?

A

8 x 12.01=96.08
10 x 1.008 = 10.08
4 x 14.01 = 56.04
2 x 16.00 = 32
add them up = 194.2 molar mass of caffeine
0.549 / 194.2 = 0.00283

37
Q

Draw the Lewis structure for NO21- and use it to answer the following questions.
1. How many valence electrons does this molecule have?
2. Select the correct description of the central atom for this molecule.
3. What is the molecular shape for this molecule?
4. Select the angle closest to that in this molecule.
5. Is this molecule polar or non-polar?

A
  1. 5+6(2)+1=18 > N=5 O=6
  2. One single bond, one double bond, and one lone pair.
  3. Bent
  4. 120
  5. Polar
38
Q

How do you find the valence electrons of a molecule?

A
  1. You take each element group number and add them.
  2. If there is ()2< you times what the group number by the outside number
39
Q

How many valence electrons does this OF2 molecule have?

A

O=6, F=7, x2
6+(7 x 2) =
6+14 = 20

40
Q

How many valence electrons does SO2 molecule have?

A

S=6, O=6, low 2 = x
6+6(2)=
6+12=18

41
Q

How many bonds are circled?

A

2

42
Q

Are these molecules polar or non-polar?

A

Polar

43
Q

Are these molecules polar or non-polar?

A
44
Q

What angle is in this molecule.

A
45
Q

What angle is in this molecule.

A
46
Q

What angle is in this molecule.

A
47
Q

What is the molecular shape?

A
48
Q

What is the molecular shape?

A
49
Q

What is the molecular shape?

A
50
Q

What is the molecular shape?

A
51
Q

What is the molecular shape?

A
52
Q

Write the formula for the following compound:
sodium phosphate

A

Na3PO4

53
Q

Write the systematic chemical name for the following compound:
Ca(NO3)2

A

calcium nitrate

54
Q

Write the systematic chemical name for the following compound:
N2O4

A

dinitrogen tetroxide

55
Q

Write the formula for the following compound:
lead (IV) oxide

A

PbO2

56
Q

Write the formula for the following compound:
sulfur dioxide

A

SO2

57
Q

How would you solve this:
The mass ratio of lead to sulfur in lead(II) sulfide is 270.0 g lead to 41.8 g sulfur. How much lead is required to completely react with 85.6 g of sulfur?

A

Line up all the element numbers
270.0g - lead
41.8g - sulfer
85.6g -sulfur
divide the known
270.0 / 41.8 =6.46
than times what is needed with number giving
85.6 x 6.46 = 553g lead

58
Q

How many hydrogen atoms are in the formula for ammonium phosphate, (NH4)3PO4?

A

NH = ammonium phosphate
So 4 x 3 = 12

59
Q

Write the chemical formula of the compound containing 2 phosphorus atoms and 5 oxygen atoms.

A
  1. 2P5O
  2. P2O5
  3. OP
  4. P2.5O
  5. P5O2
60
Q

What is the total number of atoms in a molecule of glucose, C6H12O6?

A

Add them up
=24

61
Q

How many different kinds of atoms are in a molecule of penicillin, C14H20N2SO4?

A

Count how many elements there are
=5

62
Q

Which element is a diatomic gas?

A

Hydrogen,
Nitrogen,
Oxygen,
Fluorine,
Chlorine

63
Q

Aluminum carbonate is considered which of the following?
1. Atomic element
2. Molecular element
3. Molecular compound
4. Ionic compound
5. Diatomic molecule

A
  1. Ionic compound
64
Q

How many elements occur as diatomic molecules?

A

7

65
Q

Sulfide

A
66
Q

Sulfite

A
67
Q

Sulfate

A
68
Q

The name of the compound PI3 is
1. phosphorus iodide.
2. monophosphorus triiodide.
3. phosphorus triiodide.
4. phosphorus(III) iodide.
5. potassium iodide.

A

3 phosphorus triiodide.

69
Q

The name of the compound NH4ClO4 is
1. ammonium chloride.
2. ammonium chlorite.
3. ammonium hypochlorite.
4. ammonium chlorate.
5. ammonium perchlorate.

A

5 ammonium perchlorate.

70
Q

The name of the compound SnO2 is

A

tin(IV) oxide

71
Q

The name of the compound PI3 is
1. phosphorus iodide.
2. monophosphorus triiodide.
3. phosphorus triiodide.
4. phosphorus(III) iodide.
5. potassium iodide.

A

3 phosphorus triiodide.

72
Q

The name of the compound HCN(aq) is
1. cyanic acid.
2. hydrogen cyanide.
3. percyanic acid.
4. hydrocyanic acid.
5. hypocyanous acid.

A

3 percyanic acid.

73
Q

The name of the compound HCl(g) is

A

hydrogen chloride.

74
Q

What is the correct formula for dinitrogen tetrahydride?

A

N2H4

75
Q

The state of matter in which molecules are widely spaced is

A

gas

76
Q

A state of matter that has a definite volume and is relatively incompressible is a
1. Solid.
2. Liquid.
3. Gas.
4. All of the above
5. Two of the above

A

5 Two of the above

77
Q

Which of the following is an element?
1. Sugar
2. Salt
3. Brass
4. Chlorine
5. Air

A

4 Chlorine

78
Q

Boiling point is an example of a

A

physical property

79
Q

How would you classify wine?
1. Pure substance—compound
2. Pure substance—element
3. Mixture—homogeneous
4. Mixture—heterogeneous
5. Pure substance—homogenous

A

3 Mixture—homogeneous

80
Q

Which of the following is a physical change?
1. Burning butane
2. Barbequing a steak
3. Decomposing water into hydrogen and oxygen gases
4. Breaking a piece of glass
5. Baking a cake

A

4 Breaking a piece of glass

81
Q

A solution is a(n)
1. element.
2. compound.
3. homogenous mixture.
4. heterogeneous mixture.
5. pure substance.

A

3 homogenous mixture.

82
Q

Which of the following possess(es) kinetic energy?
1. A ball falling through the air
2. A dart thrown at a dart board
3. A ball rolling down a slide
4. An arrow flying through the air
5. All of the above

A

5 All of the above

83
Q

How many kJ of energy are in a fast food hamburger containing 560. Calories? 
(Note: 1 cal = 4.184 J)
1. 2.34 kJ
2. 5.60 kJ
3. 2.34 x 103 kJ
4. 2.34 x 106 kJ
5. 5.60 x 103 kJ

A
  1. / 1000 = 0.56
    0.56 x 4.184=
    2.43 x 10^3kj
84
Q

Matter can be defined as

A

anything that has mass and occupies space.

85
Q

Which of the following changes is endothermic?

A

Water evaporates.

Intro to Chemistry (1 decks)

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