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chemistry > first test > Flashcards

first test Flashcards

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1
Q

Matter

A

anything that has mass and takes up space

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2
Q

mass

A

amount of matter that an object contains

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3
Q

mass v. Weight

A

weight is the measure of pull of gravity on object and mass is amount of matter the object contains - mass is constant throughout universe and weight is subjective to where you are in the universe

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4
Q

Volume

A

the amount of space an object takes up

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5
Q

what does matter make up

A

everything

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6
Q

how can properties of matter classified?

A

they can be classified as intensive or extensive

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7
Q

Extensive Properties

A

extensive property is a property that depends on the amount of matter in a sample, such as mass and volume

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8
Q

Intensive Properties

A

property that depends on type of matter in sample, not amount of matter - every sample of a given substance should have the same intensive properties

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9
Q

Substance

A

matter that has a uniform and definite composition

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10
Q

pure substance

A

contains only one type of matter(is NOT a mixture, one type of element, or compound ) basically only one type of particle

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11
Q

Physical property

A

condition or quality of a substance that can be measured or observed while not making any chemical changes to the substance - physical changes are ok

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12
Q

examples of physical properties (7)

A

(hardness, color, conductivity, malleability, Density, Melting Point, Solubility)

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13
Q

3 states of matter

A

solid liquid gas

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14
Q

solid(4)

A
  • particles packed close together
  • almost in-compressible,
  • expands only slightly when heated,
  • shape does not depend on shape of container
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15
Q

Liquid (5)

A
  • particles contact one another but not packed in rigid arranged
  • almost incompressible
  • expand moderately when heated
  • has no independent shape, takes on shape of its container
  • it can flow
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16
Q

Gas (3)

A
  • has indefinite volume and shape
  • it is compressible
  • Expands greatly when heated
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17
Q

Vapor

A

substance in its gaseous state that is ordinarily a liquid or solid at room temperature

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18
Q

Physical change

A

some properties of material can change, but composition does not change

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19
Q

liquid to gas transition

A

evaporation

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20
Q

what are the two types of physical changes?

A

reversible or irreversible

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21
Q

gas to liquid transition

A

condensation

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22
Q

solid to liquid transition

A

melting

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23
Q

liquid to solid transition

A

freezing

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24
Q

solid to gas transition

A

sublimation

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25
Q

gas to solid transition

A

deposition

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26
Q

mixture

A

physical blend of two or more substances - can be physically separated into its components

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27
Q

what are the two types of mixtures?

A

heterogeneous and homogenous

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28
Q

heterogeneous mixtures

A

have not uniform composition mixture

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29
Q

homogenous mixtures

A

uniform composition mixture

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30
Q

solution

A

homogenous mixture

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31
Q

element

A

substance that cannot be broken down into simpler substances under normal laboratory conditions - simplest forms of matter

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32
Q

compound(3)

A

-substance that can be separated into simpler substances only by chemical reactions, consist of two or more elements.
- generally properties of compounds are different than that of their component elements.
- specific compound always made up of same elements in same proportion

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33
Q

chemical properties

A

ability of substance to undergo chemical reactions and form new substances - only observed when substance undergoes chemical change and results in change of chemical composition

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34
Q

law of conservation of mass

A

total mass of reactants is always equal to total mass of products, quantity of matter is unchanged

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35
Q

Democritus

A

ancient philosopher, suggested existence of atoms, believed they were indivisible and indetructible

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36
Q

Dalton’s atomic theory main points(5)

A

1) Everything is composed of atoms, which are the indivisible building blocks of matter and cannot be destroyed
2) all Atoms of an element are identical
3) the Atoms of different elements vary in size and mass
4)compounds are produced through different whole-number combination of atoms
5)chemical reactions results in rearrangement of atoms in the reactant and product compounds

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37
Q

Cathode ray tube

A

sealed gas tube with near vacuum with two electrodes, when voltage is applied accross them a cathode ray beam occurs

38
Q

cathode rays

A

stream of electrons travelling from one end of cathode ray to another

39
Q

JJ Thomson’s experiemnt

A

studied cathode ray tubes, believed particles (electrons) must be negative, he said they must be part of all atoms

40
Q

what was JJ Thomson’s atom model

A

plum pudding, which was like a cloudy positive particle with negative electrons in it

41
Q

Milikan’s oil drop experiment

A

measured charge of electron by having an electric field between metal plates, and speed at which oil drops fell in different voltages helped him figure out the charge of an electron

42
Q

Rutherford

A

proved thomson’s model incorrect, used gold foil experiment to show existence of protons and the atomic nucleus

43
Q

Gold Foil Experiment

A

used beam of positively charged alpha particles(2 protons and 2 neutrons) and shot at very thing piece of gold foil, studied scattering of particles using screen behind foil, he found that the particles rarely were deflected, meaning the positive bodies within the gold atoms in the foil (neuclei) must be really small for them to be hit, most alpha particles passed through gold foil, showing how much of atom must be empty space.

44
Q

conclusions from golf foil experiment(2)

A
  1. volume occupied by atom must consist of large amount of empty space
  2. small, relatively heavy, positively charged body (nucleus) must be at the center of every atom
45
Q

Bohr’s atomic model

A

said electrons traveled in orbits around nucleus, and that chemical properties were determined by the number of electrons in the outer orbits

46
Q

chadwik

A

discovered neutrons with oscilloscope, found they were slightly heavier than protons and had neutral charge

47
Q

purpose of neutrons

A

to help reduce repulsion between protons to stabilize atom’s nucleus

48
Q

quarks

A

composes protons and neutrons, held together by color force

49
Q

what is the strong force a byproduct of

A

the color force

50
Q

how are protons and neutrons held together

A

the strong force (gluons)

51
Q

what is the mass of a neutron/proton (roughly) ?

A

1.97*10^-24 grams

52
Q

proton

A

positively charged subatomic particle forming part of nucleus of an atom, determines atomic number of an element

53
Q

neutron

A

subatomic particle forming part of nucleus, no charge

54
Q

mass of an electron

A

weigh only 9.11*10^28 grams, usually negligible

55
Q

atomic mass

A

average masses of isotopes based on their abundance

56
Q

Atomic number

A

number of protons in an element

57
Q

mass number

A

number of protons + number of neutrons

58
Q

atomic mass unit

A

1/12th mass of carbon- 12 atom?

59
Q

mendeleev’s periodic table

A

ordered in terms of relative mass, realized properties of elements related to mass in “periodic” way, arranged them so properties fell together

60
Q

moseley

A

discovered that energy of x-rays got larger with each element, proposed it was function of positive charge in nucleus, rearranged periodic table to atomic number instead of mass

61
Q

periodic law

A

states properties of elements recur in systematic way when elements are arranged in order of increasing atomic number

62
Q

horizontal rows in periodic table

A

periods

63
Q

vertical rows in periodic table

A

groups

64
Q

how many periods are there in the periodic table

A

7

65
Q

groups/famlies

A

arranged so elements in groups have same number of valence electrons

66
Q

valence electrons

A

electrons in outer most shell, that can be gained or lost in chemical reaction

67
Q

metals

A

elements that have high electrical conductivity, high luster when clean

68
Q

non-metals

A

elements that are poor conductors of electricity and are non-lustous when clean

69
Q

metalloids

A

intermediate properties between those of metals and nonmetals

70
Q

alkali metals

A

group 1 (IA) of periodic table, shiny, soft, highly reactive metals,

71
Q

Alkali earth metals

A

belong to group 2 (llA)
alkali earth metals are shiny, silvery white, low density, somewhat reactive

72
Q

general groups in A type elements

A

metals, non-metals, metalloids

73
Q

transition metals

A

group B elements, are high density, hard, high melting/boiling points

74
Q

isosagens

A

belong to group 13 (lllA)

75
Q

tetragens

A

elements that belong to group 14 (lV) of periodic table

76
Q

Pnictogens

A

group 15 (VA)

77
Q

Chalcogens

A

group 16 (VlA)

78
Q

Halogens

A

Group 17 (VllA) all nonmetals, highly reactive

79
Q

Noble Gases

A

group 18 (VlllA) all odorless, colorless, and nonmetals

80
Q

types of inner transition metals

A

lanthanides and actinides

81
Q

lanthanides

A

period 6, atomic numbers 57-71, known as rare earth metals

82
Q

Actinides

A

period 7, all radioactive, atomic numbers 89-103,

83
Q

representative elements

A

elements within groups (lA, llA, lllA, lVA, VA, VlA, VllA, VlllA) - all group A elements

84
Q

who discovered isotopes

A

Francis Aston discovered that there were three types of hydrogen atoms, called them isotopes

85
Q

isotopes

A

atoms of same elements with different numbers of neutrons, isotopes still have very similar physical properties

86
Q

half-life

A

time it takes for half of a sample of an isotope to decay

87
Q

radiocarbon dating

A

using how much Carbon 14 has deteriorated in an object to tell how old it is

88
Q

radioactive isotopes

A

isotopes that throw off radiation in an effort to become more stable

89
Q

Alpha radiation

A

composed of heavy particles, consisting of two protons and two neutrons

90
Q

Beta radiation

A

consists of electrons

91
Q

gamma radiation

A

consists of photons

92
Q

isotopes of carbon

A

carbon 12(98.9), 13(1.1), 14 (<0.1) decreasingly abundant.

chemistry (6 decks)

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