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Chemistry Semester 1 Final Flashcards > Semester 1 Flashcards > Flashcards

Semester 1 Flashcards

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1
Q

What is a compound?

A

A pure substance made of two or more elements that are chemically bonded.

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2
Q

What is a mixture?

A

A blend of any two or more kinds of matter where each maintains its own unique properties.

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3
Q

Is mass an extensive or an intensive property?

A

Extensive.

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4
Q

Is color an extensive or intensive property?

A

Intensive.

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5
Q

Is density an extensive or intensive property?

A

Intensive.

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6
Q

Is boiling point an extensive or intensive property?

A

Intensive.

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7
Q

Is volume an extensive or intensive property?

A

Extensive.

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8
Q

What is an extensive property?

A

An extensive property is a property of matter that changes as the amount of matter changes.

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9
Q

What is an intensive property?

A

Intensive properties are bulk properties, which means they do not depend on the amount of matter that is present

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10
Q

What is a physical change?

A

A change affecting the form of a chemical substance, but not its chemical composition. (Folding, melting, cutting)

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11
Q

What is a chemical change?

A

Occurs when a substance combines with another to form a new substance. (Burning wood, cooking an egg, rotting banana)

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12
Q

How are compounds separated? And what do they require?

A

Chemically. They require heat, light, or electricity.

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13
Q

How are mixtures separated?

A

Physically.

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14
Q

What is distillation?

A

Separates mixtures based on boiling points.

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15
Q

What is chromatography?

A

Separates mixtures based on their nature of pigment.

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16
Q

What is filtration?

A

Separates mixtures by separating insoluble solids from a liquid.

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17
Q

What is a homogenous mixture?

A

A homogeneous mixture is a mixture in which the composition is uniform throughout the mixture.

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18
Q

What is a heterogenous mixture?

A

A heterogeneous mixture is a mixture in which the composition is not uniform throughout the mixture.

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19
Q

How are a solid’s particles arranged?

A

They are tightly packed.

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20
Q

How are a liquid’s particles arranged?

A

They are spread out along the bottom.

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21
Q

How are a gases’ particles arranged?

A

They are very spread apart and all over the place.

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22
Q

What are the different phase changes that matter can go through? And which ones are exothermic? Endothermic?

A

Exothermic: Freezing, condensing, and desposition
Endothermic: melting, boiling, sublimation

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23
Q

What does it mean to be endothermic?

A

Heat is required to go through a phase change.

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24
Q

What does it mean to be exothermic?

A

Heat is released to go through a phase change.

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25
Q

What is chemistry the study of?

A

Matter.

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26
Q

What is matter?

A

The material of the universe: anything that takes up space and has mass.

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27
Q

What can atoms of the same elements differ in?

A

Mass number.

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28
Q

What is most of an atom’s volume made up of?

A

The electron cloud.

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29
Q

What does the atomic number tell you about the atom?

A

The number of protons.

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30
Q

What does the mass number tell you about the atom?

A

The number of protons plus neutrons.

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31
Q

What is the difference between the mass number and the atomic mass?

A

The mass number is unique to each isotope of an element. The atomic mass is the weighted average of all isotopes of an atom.

32
Q

What are ions?

A

They are atoms with the same number of protons but different number of electrons.

33
Q

What are isotopes?

A

They are atoms with the same number of protons but different number of neutrons.

34
Q

What was Dalton’s contribution to the atom?

A

The “Billiard Ball Model”-

  • All elements are made of atoms
  • All atoms of a given element are identical
  • Compounds are formed when atoms of different elements combine
  • Chemical reactions involve the rearrangement of atoms.
35
Q

What was Thompson’s contribution to the atom?

A

The “Plum Pudding Model”-

  • Discovered the electron
  • Described the atom as a sphere of positive charge with negative embedded in it
36
Q

What was Rutherford’s contribution to the atom?

A

The “Nuclear Model”-

  • Discovered the nucleus
  • The nucleus is small, dense, and positively charged
  • Most of the atom is empty space
37
Q

What was Bohr’s contribution to the atom?

A

The “Planetary Model”-

-The electrons move around the nucleus much like the planets move around the sun

38
Q

What postulate of Dalton’s theory is no longer valid and why?

A

That all atoms of a given element are identical because we know that there are different isotopes of an element. (meaning they aren’t identical)

39
Q

What is Radioactive Decay?

A

The process by which an unstable atom’s nucleus spontaneously changes by emitting ionization radiation and/ or decay particles.

40
Q

What is electromagnetic force?

A

When two like charges repel from one another.

41
Q

What is strong force?

A

t is responsible for binding together the fundamental particles of matter to form larger particles.

42
Q

Lighter isotopes are stable with a _____ ratio.

A

1:1.

43
Q

Heavier isotopes are stable with a _____ ratio.

A

1.5:1 (neutrons to protons)

44
Q

What is the penetration power of alpha, beta, and gamma particles?

A

Alpha: penetrates least.
Beta: penetrates moderately.
Gamma: penetrates most.

45
Q

What is a half life?

A

The amount of time it takes for half of a radioactive sample to decay.

46
Q

What is fission?

A

The splitting of one nucleus into many, smaller stable nuclei.

47
Q

What is fusion?

A

The combination of two smaller nuclei into one.

48
Q

What is the relationship between the frequency and the wavelength of a wave?

A

They are inversely related.

49
Q

What is the relationship between energy and the frequency of a wave?

A

They are directly related.

50
Q

What is wavelength?

A

The distance from peak to peak of a wave measured in meters.

51
Q

What is frequency?

A

The number of waves per second measured in Hertz

52
Q

What color of the visible spectrum has the lowest frequency?

A

Red.

53
Q

What is a line spectrum?

A

Voltage applied to elemental gases at reduced pressure results in a line spectrum.

54
Q

What is a continuous spectrum?

A

White light sources produce radiation containing many different wavelengths.

55
Q

What does it mean to be quantized?

A

When electrons jump from their ground state to an excited or relax back down to their relaxed state.

56
Q

Rank these in increasing wavelength: Visible light, x-rays, radio waves, gamma rays, microwaves, infrared, and ultraviolet.

A

Gamma, X-rays, UV, Visible, IR, Microwaves, radio waves

57
Q

What is an electron configuration?

A

A simple way of writing down the locations of all electrons in an atom.

58
Q

What is the Aufbau principle?

A

Energy levels fill from lowest to highest energy.

59
Q

What is the Pauli Exclusion Principle?

A

Each orbital can hold 2 electrons max and they must have opposite spin.

60
Q

What is Hund’s rule?

A

Electrons don’t pair up unless they have to.

61
Q

What is the shell?

A

The energy level.

62
Q

What is the sub shell?

A

The shape of the orbital (s, p, d, f)

63
Q

What is the orbital?

A

The orientation in space.

64
Q

What is the noble gas notation?

A

An abbreviated version of the electron configuration.

65
Q

Why do elements in the same family have similar properties?

A

They have the same number of valence electrons.

66
Q

The _____ the metal, the more reactive.

A

Larger.

67
Q

The _____ the nonmetal, the more reactive.

A

Smaller.

68
Q

What is the octet rule?

A

Having a full outer energy level, like a noble gas.

69
Q

What is the goal for every atom?

A

To be as stable as possible.

70
Q

How do cations relate to their parent atom?

A

They are smaller.

71
Q

How do anions relate to their parent atom?

A

They are larger.

72
Q

Why do atoms form bonds?

A

To be stable.

73
Q

What is an ionic bond?

A

The electrical attraction between the oppositely charged ions. (Typically a metal and nonmetal) Large difference in electronegativity.

74
Q

What is a covalent bond?

A

The mutual attraction of each atom’s nuclei to be shared valence electrons. (Typically a nonmetal and nonmetal with small to moderate difference in electronegativity)

75
Q

What type of bond has a < 0.3 electronegativity difference?

A

Nonpolar covalent

76
Q

What type of bond has a 0.3-1.7 electronegativity difference?

A

Polar Covalent

77
Q

What type of bond has a > 1.7 electronegativity difference?

A

Ionic

Chemistry Semester 1 Final Flashcards (1 decks)

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