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Chemistry Semester 1 Final Flashcards > Semester 1 Flashcards > Flashcards

Semester 1 Flashcards

(77 cards)

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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
What is chemistry the study of?
Matter.
26
What is matter?
The material of the universe: anything that takes up space and has mass.
27
What can atoms of the same elements differ in?
Mass number.
28
What is most of an atom's volume made up of?
The electron cloud.
29
What does the atomic number tell you about the atom?
The number of protons.
30
What does the mass number tell you about the atom?
The number of protons plus neutrons.
31
What is the difference between the mass number and the atomic mass?
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
What are ions?
They are atoms with the same number of protons but different number of electrons.
33
What are isotopes?
They are atoms with the same number of protons but different number of neutrons.
34
What was Dalton's contribution to the atom?
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
What was Thompson's contribution to the atom?
The "Plum Pudding Model"- - Discovered the electron - Described the atom as a sphere of positive charge with negative embedded in it
36
What was Rutherford's contribution to the atom?
The "Nuclear Model"- - Discovered the nucleus - The nucleus is small, dense, and positively charged - Most of the atom is empty space
37
What was Bohr's contribution to the atom?
The "Planetary Model"- | -The electrons move around the nucleus much like the planets move around the sun
38
What postulate of Dalton's theory is no longer valid and why?
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
What is Radioactive Decay?
The process by which an unstable atom's nucleus spontaneously changes by emitting ionization radiation and/ or decay particles.
40
What is electromagnetic force?
When two like charges repel from one another.
41
What is strong force?
t is responsible for binding together the fundamental particles of matter to form larger particles.
42
Lighter isotopes are stable with a _____ ratio.
1:1.
43
Heavier isotopes are stable with a _____ ratio.
1.5:1 (neutrons to protons)
44
What is the penetration power of alpha, beta, and gamma particles?
Alpha: penetrates least. Beta: penetrates moderately. Gamma: penetrates most.
45
What is a half life?
The amount of time it takes for half of a radioactive sample to decay.
46
What is fission?
The splitting of one nucleus into many, smaller stable nuclei.
47
What is fusion?
The combination of two smaller nuclei into one.
48
What is the relationship between the frequency and the wavelength of a wave?
They are inversely related.
49
What is the relationship between energy and the frequency of a wave?
They are directly related.
50
What is wavelength?
The distance from peak to peak of a wave measured in meters.
51
What is frequency?
The number of waves per second measured in Hertz
52
What color of the visible spectrum has the lowest frequency?
Red.
53
What is a line spectrum?
Voltage applied to elemental gases at reduced pressure results in a line spectrum.
54
What is a continuous spectrum?
White light sources produce radiation containing many different wavelengths.
55
What does it mean to be quantized?
When electrons jump from their ground state to an excited or relax back down to their relaxed state.
56
Rank these in increasing wavelength: Visible light, x-rays, radio waves, gamma rays, microwaves, infrared, and ultraviolet.
Gamma, X-rays, UV, Visible, IR, Microwaves, radio waves
57
What is an electron configuration?
A simple way of writing down the locations of all electrons in an atom.
58
What is the Aufbau principle?
Energy levels fill from lowest to highest energy.
59
What is the Pauli Exclusion Principle?
Each orbital can hold 2 electrons max and they must have opposite spin.
60
What is Hund's rule?
Electrons don't pair up unless they have to.
61
What is the shell?
The energy level.
62
What is the sub shell?
The shape of the orbital (s, p, d, f)
63
What is the orbital?
The orientation in space.
64
What is the noble gas notation?
An abbreviated version of the electron configuration.
65
Why do elements in the same family have similar properties?
They have the same number of valence electrons.
66
The _____ the metal, the more reactive.
Larger.
67
The _____ the nonmetal, the more reactive.
Smaller.
68
What is the octet rule?
Having a full outer energy level, like a noble gas.
69
What is the goal for every atom?
To be as stable as possible.
70
How do cations relate to their parent atom?
They are smaller.
71
How do anions relate to their parent atom?
They are larger.
72
Why do atoms form bonds?
To be stable.
73
What is an ionic bond?
The electrical attraction between the oppositely charged ions. (Typically a metal and nonmetal) Large difference in electronegativity.
74
What is a covalent bond?
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
What type of bond has a < 0.3 electronegativity difference?
Nonpolar covalent
76
What type of bond has a 0.3-1.7 electronegativity difference?
Polar Covalent
77
What type of bond has a > 1.7 electronegativity difference?
Ionic

Chemistry Semester 1 Final Flashcards (1 decks)

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