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Fall 2024 > Chem test 1 > Flashcards

Chem test 1 Flashcards

1
Q

What is chemistry?

A

The study of matter and the changes it undergoes

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2
Q

In practice, there is a lot of _______ between the various chemical disciplines

A

Crossover

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3
Q

What is matter?

A

Anything that has mass and occupies space

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4
Q

What are atoms?

A

submicroscopic particles that are the fundamental “building blocks” of all matter

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5
Q

What are protons?

A

positively charged particle

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6
Q

What are neutrons?

A

electrically neutral particle with about the same mass as a proton

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7
Q

What are electrons?

A

a negatively charged particle with very small mass

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8
Q

What is a molecule?

A

Two or more atoms joined together

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9
Q

If matter is comprised of a pure substance and cannot be separated into simpler subunits, then that matter is called an

A

element

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10
Q

if matter is a pure substance and is composed of two or more elements then the matter is called a

A

compound

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11
Q

if matter is consisting of 2 or more pure substances and has a uniform composition and properties, the matter is called

A

homogenous mixture

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12
Q

if matter is consisting of 2 or more pure substances and has a composition and properties that are not uniform, the matter is called a

A

Heterogeneous mixture

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13
Q

Define deposition

A

from a gas to a solid (think frost)

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14
Q

Define sublimation

A

from a solid to a gas (think dry ice)

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15
Q

What are the properties displayed in a physical change?

A

MOCTAB
melting point
odor
color
taste
appearance
boiling point

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16
Q

What are the properties displayed in a chemical change?

A

FACT
Flammability
Acidity
Corrosiveness
Toxicity

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17
Q

Who developed the atomic theory?

A

John Dalton 1808

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18
Q

What is the atomic theory?

A
  1. each element is composed of atoms
  2. all atoms of a given element have the same mass and other properties that distinguish them from other atoms in other elements
  3. atoms combine in simple, whole number ratios
  4. Atoms cannot change into atoms of another element, they just change how they are bound to create a new substance
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19
Q

Where and how are protons and neutrons bound?

A

In the nucleus by a strong nuclear forces

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20
Q

How are electrons bound to the nucleus?

A

By electromagnetic forces (opposites attract)

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21
Q

Group 1 of the periodic table are

A

alkali metals

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22
Q

group 2 of the periodic table are the

A

alkaline earth metals

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23
Q

group 3-12 are the

A

transition metals

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24
Q

group 17 are the

A

hallogens

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25
Q

group 18 are the

A

noble gasses

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26
Q

The atomic number shows

A

the number of protons in an element. Also equal to the number of electrons in an element

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27
Q

the mass number is

A

the sum of the number of protons and neutrons

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28
Q

atomic mass is

A

the average mass of an element based off of the masses of all of the isotopes that make up the element. Weighted according to the natural abundance of each isotope

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29
Q

molar mass is

A

the mass of a given element divided by the amount of substance
The mass of 1 molecules of any substance

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30
Q

The group number tells us how many ______ there are

A

valence electrons

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31
Q

What are the metalloids?

A

Boron
Silicon
Arsenic
Tellurium
Astatine
Germanium
Antimony

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32
Q

What does electron configuration tell us?

A

The exact orbital occupied by electrons within an atom. It us used to calculate the probability of finding an electron in a specific region around the nucleus.

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33
Q

What are the 3 electron configuration shapes we talked about?

A

S- sphere
P- figure 8
D- 4 leaf clove

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34
Q

What are core electrons?

A

Electrons found in the innermost circles to the the nucleus. These are the lowest energy levels

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35
Q

What are valence electrons?

A

Electrons found in the outermost circles to the the nucleus. These are the highest energy levels

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36
Q

What is the Aufbau principle?

A

Electrons are placed into the lowest energy orbitals first.

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37
Q

How do you find the number of neutrons?

A

Subtract the atomic number from the atomic mass.

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38
Q

how many electrons can the s orbital hold?

A

2

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39
Q

how many electrons can the p orbital hold?

A

6

40
Q

how many electrons can the d orbital hold?

A

10

41
Q

How can you double check that you have added the correct number of electrons to your electron configuration?

A

add all of the hyperscript numbers. this should equal the number of electrons.

42
Q

How do you know which electrons in the electron configuration are valence electrons?

A

These are the electrons found in the highest energy levels. You can find the number of valence electrons by looking at the group number (groups 13-18 subtract 10)

43
Q

If your isotope configuration is the same configuration as a noble gas, how do you write the noble gas shortcut?

A

By using the previous noble gas in brackets and listing all of the electron orbitals after that.

44
Q

An atom that has gained an electron is called an

A

anion (nonmetal)

45
Q

In anions you have to _____ electrons to your configuration

A

add

46
Q

An atom that has lost an electron is called a

A

Cation (metal)

47
Q

In cations you have to _____ electrons to your configuration

A

subtract

48
Q

What are the atomic size trends?

A

INCREASES down and to the left

49
Q

What are the electronegativity trends?

A

DECREASES down and to the left

50
Q

What is electronegativity?

A

the ability to attract electrons

51
Q

Br

A

Bromine

52
Q

I

A

Iodine

53
Q

Fe

A

Iron

54
Q

Co

A

Cobalt

55
Q

Ni

A

Nickel

56
Q

Cu

A

Copper

57
Q

Zn

A

Zinc

58
Q

Ag

A

silver

59
Q

Au

A

gold

60
Q

Pt

A

platinum

61
Q

Hg

A

mercury

62
Q

Ti

A

Titanium

63
Q

Mn

A

Manganese

64
Q

Sn

A

Tin

65
Q

Pb

A

Lead

66
Q

Cr

A

chromium

67
Q

Cs

A

cesium

68
Q

Sr

A

strontium

69
Q

Ba

A

barium

70
Q

What is the empirical formula?

A

simplest whole number ratio of a compound

71
Q

what is the molecular formula?

A

exact number of each type of atom found in a compound

72
Q

what is a structural formula?

A

exact manner in which the exact number of each type of atom is bound together

73
Q

How to find the empirical formula from a structural and molecular formula.

A

From a structure determine each type of element in the structure.
Count the amount of each type.
Arrange in the CHXNOS arrangement
This is the molecular formula.
If you can reduce each element by the same whole number then do so
this is the empirical formula.

74
Q

What is a molecular element?

A

More than one of the same element. (O2)

75
Q

Ionic compounds are composed of one or more _______ and one or more ______

A

Metals (cation) and Nonmetals (anion)

76
Q

H

A

Hydrogogen

77
Q

He

A

Helium

78
Q

Li

A

Lithium

79
Q

Be

A

Beryllium

80
Q

B

A

Boron

81
Q

C

A

Carbon

82
Q

N

A

Nitrogen

83
Q

O

A

Oxygen

84
Q

F

A

Fluorine

85
Q

Ne

A

Neon

86
Q

Na

A

Sodium

87
Q

Mg

A

Magnesium

88
Q

Al

A

Aluminum

89
Q

Si

A

Silicon

90
Q

P

A

Phosphorus

91
Q

S

A

Sulfur

92
Q

Cl

A

Chlorine

93
Q

Ar

A

Argon

94
Q

K

A

Potassium

95
Q

Ca

A

Calcium

96
Q

Molecular compounds are two or more _________

A

nonmetals

Fall 2024 (86 decks)

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