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High School Chemistry > 2017 Chemistry Final > Flashcards

2017 Chemistry Final Flashcards

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1
Q

This layer of the atmosphere contains the ozone layer.

A

Stratosphere

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2
Q

What is acid rain? (Include pH, names and formulas of the acids responsible for acid rain).

A

pH < 5.6. Sulfuric acid (H2SO4), Sulfurous acid (H2SO3), Nitric acid (HNO3), and Nitrous acid (HNO2)

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3
Q

Hydrogen bonds are formed between hydrogen and these elements:____

A

N, O, and F

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4
Q

When a compound is formed by 2 elements, its name will end in this:

A

-ide

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5
Q

Pressure is measured by this instrument:

A

Barometer

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6
Q

The volume of liquids is measured in this type of lab equipment:

A

Graduated cylinder

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7
Q

What is an aqueous solution with a high OH- concentration?

A

A base

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8
Q

Hexane and water will not mix. What type of bond makes hexane?

A

Hexane is made of non-polar covalent bonds which are not soluble in water which is polar.

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9
Q

How many molecules in one mol of H2SO4?

A

6.02*10^23 molecules

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10
Q

Give 3 properties of gases.

A

Here are four:

  1. Compressible
  2. Low density
  3. Fluid
  4. Fills their container
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11
Q

Define activated complex

A

An unstable structure that represents the transition between the breaking of old bonds and the formation of new bonds.

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12
Q

Define surface tension.

A

Cohesion of the water molecules due to hydrogen bonding

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13
Q

List 3 properties of water that are unexpectedly different due to hydrogen bonding.

A
  1. Higher boiling points
  2. Low vapor pressure
  3. High surface tension
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14
Q

Define solution and give 2 examples.

A

A mixture between a solvent and a solute.

  1. Salt water
  2. CuSO4
  3. Gasoline
  4. Air
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15
Q

What is the molar volume of any gas at STP?

A

22.4 L

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16
Q

In a chemical reaction, if the heat content of the reactants is less than that of the products, would the reaction be exothermic or endothermic?

A

Endothermic

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17
Q

Name 2 of the most common gases in our atmosphere and give their percentages

A 
N2 = 78%
O2 = 21%
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18
Q

Which elements are diatomic?

A
  1. H2
  2. N2
  3. O2
  4. F2
  5. Cl2
  6. Br2
  7. I2
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19
Q

Name five things that affect reaction rate.

A
  1. Nature of the reactants
  2. Temperature
  3. Concentration
  4. Surface area
  5. Catalyst
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20
Q

Define calorie.

A

The amount of energy to raise the temperature of 1 g of water by 1 degree celsius

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21
Q

States Charles’ Law

A

Temperature is directly proportional to volume (V1/T1) = (V2/T2)

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22
Q

Write the chemical name for FeCl2

A

Iron (II) Chloride

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23
Q

Write the formula for Barium Nitrate

A

Ba(NO3)2

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24
Q

What is the difference between a saturated and unsaturated fat?

A

Saturated has no double C=C bonds, while unsaturated fats have at least 1 double C=C bond

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25
Q

What is meant by products and reactants?

A

Products are formed when reactants react

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26
Q

What are 5 basic types of reactions?

A
  1. Single replacement
  2. Double replacement
  3. Decomposition
  4. Synthesis
  5. Combustion
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27
Q

What 2 products are always formed in the combustion of a hydrocarbon?

A
  1. Water (H2O)

2. Carbon Dioxide (CO2)

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28
Q

Which side of the arrow will the energy term be placed when representing an exothermic reaction and what sign will the (delta)H be?

A

Product side. (Delta)H is negative.

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29
Q

What is activation energy?

A

The minimum amount of energy needed for a reaction to occur.

30
Q

If (delta)H is negative, is the reaction endothermic or exothermic?

A

Exothermic.

31
Q

What factors affect equilibrium?

A
  1. Concentration
  2. Temperature
  3. Pressure
32
Q

Give the definition for Buffer system.

A

A buffer consists of a weak acid and base and resists the change in pH with small additions of an acid or base.

33
Q

Differentiate between an unsaturated, saturated, and supersaturated solution.

A

Unsaturated solution will dissolve more solute.
Saturated solution will not dissolve more solute.
Supersaturated solution will crystalize when more solute is added.

34
Q

Define an alloy and give an example

A

An alloy is a solution between 2 solids

  1. Brass
  2. Bronze
  3. Steel
35
Q

Orange juice with pulp is this type of mixture.

A

Suspension

36
Q

What part of a CFC molecule is harmful to the ozone layer? Why?

A

Chlorine is harmful because it reacts with O2 to form atmospheric oxygen. It catalyzes the destruction of the ozone layer.

37
Q

Define pressure.

A

Pressure = Force/Unit area

38
Q

What are the products of a neutralization reaction?

A

Water and salt

ex. HCl + NaOH –> H2O + NaCl

39
Q

Define catalyst.

A

A substance that speeds up a reaction without getting used up

40
Q

Name the factor that affects solubility.

A

Temperature

41
Q

When is chemical equilibrium reached?

A

When the forward and reverse reaction rates are equal.

42
Q

On a scale of 1 to 10, how well are you going to do on this test?

A

10

43
Q

Define heat

A

The degree of temperature being transferred from water to cool subtance

44
Q

Define temperature

A

amount of kinetic energy in substance

45
Q

What is the name of Ca(ClO3)2?

A

Calcium chlorate

46
Q

What is the name of MnO2

A

Manganese (IV) oxide

47
Q

What is the name of CCl4

A

Carbon tetrachloride

48
Q

What is the name of KMnO4

A

Potassium Permanganate

49
Q

What are the values for standard temperature and standard pressure when it comes to gas laws?

A

0 C and 273 K

1 atm and 101.325 kPa

50
Q

Define specific heat

A

The amount of energy needed to raise the temperature of 1 g of a substance 1 C.

51
Q

Define molar volume.

A

The volume of 1 mole of gas at STP.

52
Q

What type of bond would you expect in MgCl2?

A

Ionic

53
Q

What type of bond would you expect in N2

A

Non-polar covalent

54
Q

What type of bond would you expect in NO2

A

Polar covalent

55
Q

Define ionic bonds

A
  1. Transfers electrons
  2. Electronegativity difference is > 1.7
  3. Between a metal atom and non-metal ion
56
Q

Define covalent bonds

A
  1. Shares electrons
  2. Electronegativity difference is < 1.7
  3. Between 2 non-metals
57
Q

Is orange juice a homogeneous substance, heterogenous substance, or pure substance?

A

Heterogeneous substance

58
Q

Name 6 properties of acids

A
  1. Reacts with carbonates to form CO2
  2. Neutralizes bases
  3. Turn blue litmus paper red
  4. Tastes sour
  5. pH < 7.0
  6. React with metals to form H2
59
Q

Name 5 properties of bases.

A
  1. Slippery
  2. Tastes bitter
  3. Neutralizes acids
  4. pH > 7.0
  5. Turns red litmus paper blue.
60
Q

Define enthalpy

A

The total energy of a system at constant pressure.

61
Q

State Dalton’s Law of Partial Pressure.

A

The total pressure of a system is equal to the sum of the individual pressures in the sample.

62
Q

Differentiate between a polar and non-polar molecule.

A

Polar molecules have an unequal distribution of charges while there is equal distribution in non-polar molecules.

63
Q

Define entropy

A

The tendency towards more disorder.

64
Q

Define standard solution

A

Solution of known concentration

Ex). 5 M of HCl or 1 M of NaOH.

65
Q

End point

A

The point where the indicator for the acid-base titration changes color.

66
Q

Acid-base titration

A

A means of determining the unknown concentration of a solution by using a standard solution. A standard solution is a solution of known concentration.

67
Q

Name 5 green houses gases and explain how they maintain our ecosystem.

A
  1. CO2
  2. CH4
  3. H2O
  4. CFCs
  5. N2O
68
Q

Name NH3

A

Ammonia

69
Q

Name CH4

A

Methane

70
Q

Name HCl

A

hydrochloric acid

71
Q

Name H2SO4

A

Sulfuric acid

High School Chemistry (7 decks)

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