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Gen Chem 1 > Midterm 1 vocab > Flashcards

Midterm 1 vocab Flashcards

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1
Q

chemistry

A

the scientific study of the properties, composition, and structure of matter, the transformations matter undergoes, and the energy of these processes

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2
Q

matter

A

anything that has mass and occupies space

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3
Q

mass

A

a measure of the amount of matter in an object

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4
Q

weight

A

a measure of the gravitational pull on an object

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5
Q

physical process

A

acts on the physical state of matter but doesn’t change its chemical identity (atoms and bonds between them remain the same)

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6
Q

molecule

A

an assembly of two or more atoms held together in a characteristic pattern by chemical bonds

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7
Q

Law of Constant Composition

A

every sample of a compound contains the same elements combined in the same proportions

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8
Q

intensive properties + example

A

properties that are independent of the amount of substance (ex. hardness, density, phase transition temperature)

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9
Q

extensive properties + example

A

properties that depend on the amount of a substance present (mass, length, width, volume, etc)

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10
Q

physical properties

A

can be determined without changing a substance into a different substance

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11
Q

chemical properties

A

can only be observed by reacting a substance to form a new substance in a chemical reaction

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12
Q

precision

A

how consistent your results are (less random error, the more precision)

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13
Q

random error

A

error that produces inconsistent measured values of a constant quantity (can only be determined from a set of at least two repeated measurements)

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14
Q

accuracy

A

how close you are to the “correct” value

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15
Q

pure substance

A

has constant composition

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16
Q

mixtures

A

composition varies by sample

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17
Q

elements

A

substances made up of one type of atom

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18
Q

compounds

A

substances made up of more than one type of atom

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19
Q

heterogeneous mixture

A

a physical combination that is not uniform

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20
Q

homogeneous mixture

A

a physical combination that is uniform

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21
Q

solids

A

have defined volume and shape

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22
Q

liquid

A

have defined volume, no definite shape

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23
Q

gas

A

no definite volume or definite shape

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24
Q

a solid ____ turns into gas

A

subliming

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25
Q

a gas _____ turns into a solid

A

depositing

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26
Q

a gas ____ turns into a liquid

A

condensing

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27
Q

heterogeneous mixtures can be separated by…

A

centrifugation or filtration

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28
Q

homogeneous mixtures can be separated by

A

distillation or evaporation

29
Q

orbitals

A

the 3D areas of space that electrons can occupy around the nucleus

30
Q

The scientific method outlines…

A

how we form and test hypotheses to create scientific theories and models

31
Q

Dimensional analysis

A

unit conversions

32
Q

scientific notation

A

a more convenient way to write out and compare very large and very small numbers

33
Q

John Dalton’s atomic theory stated

A

elements are made of indivisible small particles called atoms; different elements are composed of different kinds of atoms

34
Q

_____ _____ dictates the properties of different elements

A

atomic structure

35
Q

What conclusion resulted from Thompson’s Cathode Ray Tube experiment?

A

electrons are negatively charged and highly charged and extremely light

36
Q

Who proposed the plum pudding model

A

Thompson

37
Q

Describe beta particles

A

have the same charge-to-mass ratio and negative charge as electrons, are therefore high-energy electrons

38
Q

Describe alpha particles

A

have twice as much charge and the opposite sign as an electron (+2) and are 10^3 times heavier

39
Q

What kind of particles did Rutherford use in his Gold Foil Experiment?

A

Alpha particles

40
Q

Describe Rutherford’s Gold Foil Experiment

A

Alpha particles were shot at a piece of gold foil and most particles passed directly through the foil, meaning most of the space in the gold foil was empty, and very rarely an alpha particle was deflected strongly from the foil, which means the gold foil also contained occasional small, dense, highly charged centers that strongly deflect alpha particles

41
Q

Describe Rutherford’s nuclear model

A

A positively charge is contained in the atomic nucleus at the center, surrounded by a diffuse cloud of negatively charged electrons

42
Q

Describe Protons

A

center of atom(nucleus), approx 1 atomic mass unit, positive charge

43
Q

atomic number equals the amount of ___

A

protons

44
Q

Describe Neutrons

A

center of atom(nucleus), approx 1 atomic mass unit, no charge

45
Q

the atomic mass number equals ____

A

neutrons + # protons

46
Q

the _____ _____ is used to tell the difference between isotopes

A

mass number

47
Q

Describe electrons

A

found outside the nucleus, approx 0 atomic mass unit, negative charge

48
Q

A neutral atom has this ratio of protons to electrons

A

equal

49
Q

if you change the number of electrons, you will form an ____

A

ion

50
Q

Cations have a ____ charge because they have more _____

A

positive, protons

51
Q

Anions have a ____ charge because they have more _____

A

negative, electrons

52
Q

The charge is written on the ____ _____ of the chemical symbol

A

upper right

53
Q

The average atomic mass equals

A

the average mass of isotope 1, and so on for the other stable elements

54
Q

Each orbital can contain up to ___ electrons

A

2

55
Q

Electrons can only exist at the discrete energy levels of the orbitals, so the energy of an electron is ____

A

quantized

56
Q

The further an electron is from the nucleus, the ____ the energy.

A

higher

57
Q

Orbitals of an atom are defined by which quantum numbers

A

n, l, ml, ms

58
Q

Amount of total nodes =

A

n - 1

59
Q

define n

A

which shell the orbital belongs to; how far away the electron is from the nucleus

60
Q

orbitals in the same shell have the same value of ___

A

n

61
Q

define node

A

an area where no electron can exist

62
Q

define radial node

A

a spherical shell that never passes through the nucleus (origin)

63
Q

define angular node

A

a plane or a cone that always pass through the nucleus

64
Q

what are the two kinds of nodes? which one passes through the nucleus, and which one doesn’t?

A

Radial and Angular; radial does not pass through the nucleus, angular does

65
Q

Nodes ____ the energy of the orbital

A

increase (the less close space to the nucleus the farther the electrons must be and therefore higher energy)

66
Q

What value equals the # of angular nodes?

A

L

67
Q

what does l define?

A

The shape of an orbital

68
Q
A

Gen Chem 1 (1 decks)

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