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Chemistry > Module 1 > Flashcards

Module 1 Flashcards

8/27/24

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1
Q

What is the definition of chemistry?

A

The study of matter and the changes it undergoes

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2
Q

What type of chemist is our professor?

A

Organic Chemist; study of carbon compounds

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3
Q

What is a Physical Chemist?

A

More theoretical than applied; uses complex math to determine chemistry.

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4
Q

What is an Analytic Chemist?

A

study of methods for quantifying matter; ex) MRI

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5
Q

What is Inorganic Chemistry?

A

Study of substances without carbon

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6
Q

What is a a Biochemist?

A

Study chemical processes within living systems.

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7
Q

What is matter?

A

Anything that has mass and occupies space

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8
Q

Does light have mass?

A

No. Light is made of photons; photons are massless

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9
Q

What are the 3 types of matter?

A

Solid, liquid, gas

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10
Q

What is a key characteristic of a solid?

A

It has a defined shape

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11
Q

What happens when you compress a solid?

A

It will break

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12
Q

Describe the arrangement of matter in a solid.

A

Ordered and tightly arranged

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13
Q

Describe the arrangement of matter in a liquid.

A

Loose and not well defined

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14
Q

Describe the arrangement of matter in a gas.

A

Lots of space and unorganized between atoms

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15
Q

What is a key characteristic of gas?

A

It is easily compressed; when you compress you decrease the volume but increase the pressure.

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16
Q

When you cool and compress a gas so much it will turn into ______

A

Liquid

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17
Q

Liquids and gas require a _______.

A

Container

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18
Q

Explain what happens when an oxygen tank is empty.

A

The pressure on the outside of the tank and on the inside have equalized. There’s still gas inside just no pressure to push it out.

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19
Q

What is an atom?

A

The “building blocks” of all matter

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20
Q

What subatomic particles make up an atom?

A

Protons, Neutrons, and electrons

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21
Q

What is a proton?

A

Positively charged particle

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22
Q

What is the atomic number?

A

Tells us the identity of an atom. Atomic number is equal to protons and electrons

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23
Q

What is a neutron?

A

Electrically neutral particle. mass almost equal to a proton. When your neutrons differ then you have an isotope.

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24
Q

How do you find the number of neutrons?

A

Mass number minus protons

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25
Q

What is an electron?

A

Negatively charged particle with a very small mass.

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26
Q

How do you find the number of electrons?

A

Protons are equal to electrons in neutrally charged elements

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27
Q

What is the nucleus of an atom?

A

Protons and neutrons in a dense core

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28
Q

Gas/non metals like to ______ an electron

A

Gain

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29
Q

Metals like to ____ an electron

A

Lose

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30
Q

What is a molecule?

A

2 or more atoms joined; can be same or different elements; Ex) O2 and H2O

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31
Q

What is a compound?

A

2 or more different elements that are chemically bonded in a fixed ratio. Ex) H2O

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32
Q

What are the 4 classifications of matter?

A

Element; Compound; Homogenous mixture; heterogenous mixture

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33
Q

How many types of matter is in a pure substance?

A

1

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34
Q

How many types of matter are in a mixture?

A

2

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35
Q

What’s the difference between a homogeneous and heterogenous mixture?

A

In a heterogenous mixture you can visually see the different types of matter; in homogenous you can not.

36
Q

What is the difference between an element and a compound

A

An element is 1 type of the same atom and cannot be broken down; A compound is 2 or more elements

37
Q

Define a physical change in matter and give an example.

A

Changes appearance but not composition. An example is H2O: Ice, water, and steam.

38
Q

Solid to a liquid is…

A

Melting

39
Q

Liquid to a Solid is…

A

Freezing

40
Q

Liquid to a gas is…

A

Vaporization

41
Q

Gas to a liquid is…

A

Condensation

42
Q

Gas to a solid is….

A

Deposition

43
Q

Solid to a gas is…

A

Sublimation

44
Q

What is a chemical change?

A

changes the composition, which changes the chemical properties; creates a new compound.

45
Q

What are the 4 aspects of the Atomic Theory and who was it developed by?

A

John Dalton.
-Each element is composed of tiny, indestructible particles called atoms
-All atoms of an element have the same mass and properties that distinguish them from other elements
-Atoms combine in simple, whole-number ratios to form compounds
-Atoms of one element cannot change into atoms of another

46
Q

Where are electrons in the atom?

A

Bound outside the nucleus by electromagnetic forces

47
Q

What group are the Noble Gasses?

A

18

48
Q

What group are the Halogens?

A

17

49
Q

Where are the Transition Elements?

A

Group 3 - 12

50
Q

What group are the Alkaline metals?

A

1

51
Q

What group are the Alkaline Earth Metals?

A

2

52
Q

What groups include the Main Group Elements?

A

1-2 and 13-18

53
Q

What is Mass Number?

A

Protons and Neutrons

54
Q

What is Molar Mass?

A

Mass of a given element divided by the amount of substance (g/mol)

55
Q

Where are the non metals located on the periodic table?

A

On the right side

56
Q

Where are the metals located on the periodic table?

A

On the left

57
Q

Where are the metalloids on the periodic table?

A

Between the metals and non metals

58
Q

What non metals are solids?

A

C, P, Se, I, S

59
Q

What is the state of matter of Mercury (Hg)

A

Liquid metal

60
Q

What is the state of matter for Bromine (Br)

A

Liquid

61
Q

What type of properties do metalloids have?

A

Metal and non metal properties

62
Q

What does the position within the periodic table show?

A

You’re able to predict properties based on location

63
Q

What determines how an element will behave?

A

Electrons

64
Q

What are atomic orbitals used for?

A

To calculate probability of finding an electron in a specific region

65
Q

Describe the 3 orbitals

A

s - sphere
p - figure eight
d - clover

66
Q

Describe Core electrons

A

Innermost: closest to nucleus
Tightly bound
Not involved in chemical bonding
Influences chemical reactivity of atom

67
Q

Describe Valence electrons

A

Outermost: farther from nucleus
Not tightly bound
Involved in chemical bonding
influences properties of atom

68
Q

How can you find the valence electrons by looking at the periodic table?

A

The group number. Once you get to group 13, subtract 10 from the group number.

69
Q

What is electron configuration?

A

A system that places electrons into the proper orbitals

70
Q

What is the Aufbau Principle?

A

Electrons are always placed into the orbital of the lowest energy available

71
Q

Describe a S-orbital in electron configuration.

A

1 orbital; 2 electrons

72
Q

Describe a P-orbital in electron configuration.

A

3 degenerate orbitals; 6 electrons total

73
Q

Describe a D-orbital in electron configuration.

A

5 degenerate orbitals; 10 electrons total

74
Q

What is the electron configuration for Calcium?

A

1s1. 2s2. 2p6. 3s2. 3p6. 4s2.

75
Q

What is the Noble Gas shortcut for Calcium?

A

[AR]4s2

76
Q

What is the Noble gas shortcut?

A

Doesn’t work for H and He
- Find the nearest noble gas and put the in brackets
- The period of that element is the prefix
- Find the number of valence electrons as exponent

77
Q

What are ions?

A

When an element lose or gains an electron because they want to adjust to the noble gas that is nearest them.

78
Q

What is an anion?

A

An ion that gained an electron and has a negative charge

79
Q

What is a cation?

A

An ion that lost an electron and has a positive charge

80
Q

What are some predictable ionic charges based off their location on the periodic table?

A

L = lose; cations (+)
Group 1 likes to lose 1 electron
group 2 likes to lose 2 electrons

Right side likes to gain; anions (-)
Group 17 likes to gain 1 electron
group 16 likes to gain 2
group 15 likes to gain 3

81
Q

What are the periodic trends if you move down groups and to the left of periods?

A

Atomic size increases
electronegativity decreases
ionization energy decreases

82
Q

What is electronegativity?

A

Ability to attract electrons

83
Q

What is the size difference of cations and anions

A

Anions are bigger than their corresponding cation

84
Q

What is ionization energy?

A

energy required to remove an electron

85
Q

What happens to ionization energy when you remove an electron?

A

Increases

Chemistry (13 decks)

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