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Chemistry > Module 1 > Flashcards

Module 1 Flashcards

8/27/24 (85 cards)

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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
What is an electron?
Negatively charged particle with a very small mass.
26
How do you find the number of electrons?
Protons are equal to electrons in neutrally charged elements
27
What is the nucleus of an atom?
Protons and neutrons in a dense core
28
Gas/non metals like to ______ an electron
Gain
29
Metals like to ____ an electron
Lose
30
What is a molecule?
2 or more atoms joined; can be same or different elements; Ex) O2 and H2O
31
What is a compound?
2 or more different elements that are chemically bonded in a fixed ratio. Ex) H2O
32
What are the 4 classifications of matter?
Element; Compound; Homogenous mixture; heterogenous mixture
33
How many types of matter is in a pure substance?
1
34
How many types of matter are in a mixture?
2
35
What's the difference between a homogeneous and heterogenous mixture?
In a heterogenous mixture you can visually see the different types of matter; in homogenous you can not.
36
What is the difference between an element and a compound
An element is 1 type of the same atom and cannot be broken down; A compound is 2 or more elements
37
Define a physical change in matter and give an example.
Changes appearance but not composition. An example is H2O: Ice, water, and steam.
38
Solid to a liquid is...
Melting
39
Liquid to a Solid is...
Freezing
40
Liquid to a gas is...
Vaporization
41
Gas to a liquid is...
Condensation
42
Gas to a solid is....
Deposition
43
Solid to a gas is...
Sublimation
44
What is a chemical change?
changes the composition, which changes the chemical properties; creates a new compound.
45
What are the 4 aspects of the Atomic Theory and who was it developed by?
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
Where are electrons in the atom?
Bound outside the nucleus by electromagnetic forces
47
What group are the Noble Gasses?
18
48
What group are the Halogens?
17
49
Where are the Transition Elements?
Group 3 - 12
50
What group are the Alkaline metals?
1
51
What group are the Alkaline Earth Metals?
2
52
What groups include the Main Group Elements?
1-2 and 13-18
53
What is Mass Number?
Protons and Neutrons
54
What is Molar Mass?
Mass of a given element divided by the amount of substance (g/mol)
55
Where are the non metals located on the periodic table?
On the right side
56
Where are the metals located on the periodic table?
On the left
57
Where are the metalloids on the periodic table?
Between the metals and non metals
58
What non metals are solids?
C, P, Se, I, S
59
What is the state of matter of Mercury (Hg)
Liquid metal
60
What is the state of matter for Bromine (Br)
Liquid
61
What type of properties do metalloids have?
Metal and non metal properties
62
What does the position within the periodic table show?
You're able to predict properties based on location
63
What determines how an element will behave?
Electrons
64
What are atomic orbitals used for?
To calculate probability of finding an electron in a specific region
65
Describe the 3 orbitals
s - sphere p - figure eight d - clover
66
Describe Core electrons
Innermost: closest to nucleus Tightly bound Not involved in chemical bonding Influences chemical reactivity of atom
67
Describe Valence electrons
Outermost: farther from nucleus Not tightly bound Involved in chemical bonding influences properties of atom
68
How can you find the valence electrons by looking at the periodic table?
The group number. Once you get to group 13, subtract 10 from the group number.
69
What is electron configuration?
A system that places electrons into the proper orbitals
70
What is the Aufbau Principle?
Electrons are always placed into the orbital of the lowest energy available
71
Describe a S-orbital in electron configuration.
1 orbital; 2 electrons
72
Describe a P-orbital in electron configuration.
3 degenerate orbitals; 6 electrons total
73
Describe a D-orbital in electron configuration.
5 degenerate orbitals; 10 electrons total
74
What is the electron configuration for Calcium?
1s1. 2s2. 2p6. 3s2. 3p6. 4s2.
75
What is the Noble Gas shortcut for Calcium?
[AR]4s2
76
What is the Noble gas shortcut?
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
What are ions?
When an element lose or gains an electron because they want to adjust to the noble gas that is nearest them.
78
What is an anion?
An ion that gained an electron and has a negative charge
79
What is a cation?
An ion that lost an electron and has a positive charge
80
What are some predictable ionic charges based off their location on the periodic table?
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
What are the periodic trends if you move down groups and to the left of periods?
Atomic size increases electronegativity decreases ionization energy decreases
82
What is electronegativity?
Ability to attract electrons
83
What is the size difference of cations and anions
Anions are bigger than their corresponding cation
84
What is ionization energy?
energy required to remove an electron
85
What happens to ionization energy when you remove an electron?
Increases

Chemistry (13 decks)

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