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Chemistry > General Chemistry Stuff > Flashcards

General Chemistry Stuff Flashcards

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1
Q

Definition of Chemistry

A

the study of matter and the changes it undergoes

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2
Q

Definition of matter

A

anything that has mass and takes up space

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3
Q

Definition of atoms

A

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

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4
Q

Physical characteristics of solid

A
  • definite shape
  • not easily compressible
  • molecules are densely packed
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5
Q

Physical characteristics of liquid

A
  • no definite shape
  • not easily compressible
  • molecules are loosely packed
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6
Q

Physical characteristics of gas

A
  • no definite shape
  • easily compressible
  • molecules not packed
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7
Q

An tank of gas becomes “empty” when -

A

the pressure inside the tank equalizes with the pressure of the atmosphere (even if there is still gas in the tank)

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8
Q

Atomic mass

A

Made up of the protons and neutrons

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9
Q

The number of protons gives us it’s___ and identifies which ___ it is

A

atomic number; element

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10
Q

What does changing the number of neutrons of an element do?

A

change the mass and creates isotopes

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11
Q

What determines the charge of the element?

A

The electrons

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12
Q

Definition of a molecule

A

two or more atoms joined together

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13
Q

Definition of a compound

A

a molecule that contains at least two different elements

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14
Q

What is matter called that consists of two or more pure substances that retain their individual identities?

A

a mixture

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15
Q

What is a pure substance that can be broken into separate parts called?

A

a compound

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16
Q

What are chemical properties of matter?

A

property displayed by a substance caused by a change in it’s composition (flammability, acidity, toxicity)

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17
Q

Where are alkali metals found?

A

Group 1

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18
Q

Where are alkaline earth metals found?

A

Group 2

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19
Q

Where are halogens found?

A

Group 17

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20
Q

Where are noble gasses found?

A

Group 18

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21
Q

Where are transition metals found?

A

Group 3-12

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22
Q

What are core electrons?

A

innermost electrons that occupy the lowest energy levels and are not involved in chemical bonding

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23
Q

What are valence electrons?

A

outermost electrons that occupy the highest energy level and are involved in chemical bonding

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24
Q

Aufbau principle

A

an electron occupies the lowest-energy orbital that can receive it

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25
Q

Trends of atomic size on periodic table

A

increases going down and to the left

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26
Q

Trends of electronegativity on periodic table

A

decreases going down and to the left

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27
Q

Empirical formula

A

the simplest whole number ratio of the elements in a compound

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28
Q

Structural formula

A

the exact number of each type of element and exact manner in which these atoms are bound together (Lewis structure)

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29
Q

Molecular formula

A

the exact numbers of each type of element found in a compound

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30
Q

Define atomic elements

A

elements that exist in nature with single atoms as their basic unit (Na, Mg, Ag, Au)

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31
Q

Define molecular elements

A

elements that exist in nature as molecules (H2, N2, O2, Cl2, Br2, P4)

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32
Q

What is a molecular compound?

A

composed of two or more non-metals

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33
Q

Melting

A

Solid–> liquid

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34
Q

Freezing

A

Liquid–> solid

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35
Q

Vaporization

A

Liquid –> gas

36
Q

condensation

A

gas–> liquid

37
Q

deposition

A

gas–> solid

38
Q

sublimination

A

solid–> gas

39
Q

Atoms

A

Submicroscopic particles that are the fundamental building blocks of all matter

40
Q

What makes up the bulk of an atoms mass?

A

Protons and neutrons

41
Q

Where are protons, neutrons and electrons located?

A

Protons and neutrons are in the nucleus.

Electrons reside in the space around atoms (electron cloud)

42
Q

What is an element?

A

Cannot be separated into simpler substance

43
Q

What is a compound?

A

Substance composed of two or more elements.

Can be separated into simpler substances/elements only by chemical methods

44
Q

What is a homogeneous mixture?

A

A mixture with uniform composition (solution)

45
Q

What is a heterogeneous mixture?

A

Mixture not uniform and composition and properties

46
Q

What is a pure substance?

A

Cannot be broken down further

47
Q

What is the chemical change?

A

A change that alters composition

Creating different substances

48
Q

Who developed the atomic theory?

A

John Dalton in 1808

49
Q

Atomic theory

A

Each element is composed of atoms

All atoms of an element have same mass and other properties that distinguish them from other atoms

Atoms combine in simple whole number ratios to form compounds

Atoms of one element cannot change into atoms of another element

50
Q

Pauli exclusion principle

A

No 2 electrons can be the same and must be paired opposite (spin paired)

51
Q

S-orbital

A

Holds 2 electrons

52
Q

P-orbital

A

3 orbitals

Holds 6 electrons

53
Q

D orbitals

A

5 orbitals

Holds 10 electrons

54
Q

F- orbitals

A

7 orbitals

holds 14 electrons

55
Q

Why do atoms gain/lose electrons?

A

To give electron configuration similar to noble gas (more stable)

56
Q

Cations

A

Lose electrons

Cations are smaller than corresponding atoms

57
Q

Anions

A

Gain electrons

Anions are bigger than corresponding atoms

58
Q

Non- metals

A

Do not conduct electricity

Ex: most gases

59
Q

Metals

A

Malleable/ductile

Conduct electricity

Usually solid (except Hg)

60
Q

Metalloids

A

Properties of both metals and nonmetals

61
Q

Neutrons

A

Isotope- number of protons

62
Q

Law of conservation of mass

A

Lavoisier—matter is neither created nor destroyed

matter is converted into other forms not destroyed

63
Q

Law of definite proportions

A

All samples of a given compound have the same proportions of their constituent elements

Ex: water (however it got there all water is 2H+ and 1O

64
Q

Toxicity

A

An example of chemical property

65
Q

Law of multiple proportions

A

When two elements form two different compounds with similar bonding

Masses of element b that combine with the same amount of element A can be expressed as a ratio of small whole number

66
Q

Example of chemical change

A

Iron rusting—iron rebinding to O2 changes chemical properties

67
Q

Diatomic elements

A

“Have No Fear Of Ice Cold Beer”

H2
N2
F2
O2
I2
Cl2
Br2

68
Q

Ionic compound

A

Metal (cation) and nonmetal (anion)

69
Q

Molecular compounds

A

2 or more nonmetals

70
Q

What is Zn ion

A

Zn2+

71
Q

What is Ag ion

A

Always Ag+

72
Q

What is the only poly atomic cation?

A

Ammonium NH4+

73
Q

How to determine ionic charge of transition metal?

A

Cation charge= -(anion subscript)(anion charge)/ (cation subscript)

74
Q

Binary acids

A

HCl: hydrochloric acid
HBr: hydrobromic acid
HI: hydroiodic acid
HF: hydrofluoric acid

75
Q

Oxoacids

A

Come from polyatomic ions

-ate goes to -ic

-ite goes to -ous

76
Q

Reducing chemical formulas

A

CAN reduce ionic compounds

CANNOT reduce molecular compounds—would change compound

77
Q

Why do atoms form bonds?

A

To lower potential energy(more stable)—high energy things are unstable

Bonds allow unpaired electrons to become paired

78
Q

Polar covalent bond

A

Electrons not shared equally

Electron density more towards most electronegative atom

79
Q

Nonpolar covalent bonds

A

Electrons are shared equally between atoms

Usually when electronegativity is low

Ex: C bonds, 2 of some element bonded together

80
Q

Exceptions to octet

A

H: 2 electrons
B: 6 electrons
Al: 6 electrons

81
Q

Expanded octets

A

Period 3 or higher

Due to D orbitals

82
Q

Lone pairs

A

Lone pairs have greater density than peripheral atoms—repel each other

83
Q

If octahedral has lone pair which axis is it drawn on

A

Lone pairs fill axial axis

84
Q

If trigonal bipyramidal have a lone pair where does it go first?

A

Equatorial axis fill with lone pairs

85
Q

Binary ionic

A

Cation and anion are both one element ex: NaCl

86
Q

Electronegativity

A

Property for bonding and reactivity

Chemistry (6 decks)

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