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9 Chemistry > 11 Atoms the Basic Unit of Matter > Flashcards

11 Atoms the Basic Unit of Matter Flashcards

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1
Q

matter is made up of

A

atoms

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2
Q

are the smallest whole particles

A

atoms

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3
Q

basic unit of matter

A

atoms

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4
Q

smaller particles that compose the atom

A

subatomic particles

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5
Q

dense central core of the atom

A

nucleus

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6
Q

subatomic particles found in the nuclei

A

nucleons

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7
Q

positively charge particle

A

protons

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8
Q

makes the identity of an atom

A

protons

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9
Q

equal to the number of protons inside the nucleus

A

atomic number

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10
Q

neutral particles

A

neutrons

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11
Q

atoms of the same element but have DIFFERENT number of neutrons

A

isotopes

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12
Q

determines the stability of the atom

A

isotopes

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13
Q

H1

A

protium

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14
Q

H2

A

deuterium

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15
Q

H3

A

tritium

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16
Q

still smaller particles that compose the protons and neutrons

A

quarks

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17
Q

According to quark theory, _____ quarks are needed to make a proton or a neutron

A

3

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18
Q

reacts and bonds with other electrons of atoms to form substances

A

electrons

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19
Q

layers; orbits; energy levels

A

electron shells

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20
Q

shells farther from the nucleus can hold
___ electrons than the innermost shells

A

more

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21
Q

greek philosopher (470 – 380 BC) who is the father of modern atomic thought

A

democritus

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22
Q

proposed that matter cannot be divided into smaller pieces forever

A

democritus

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23
Q

claimed that matter was made of small, hard particles called “atomos”

A

democritus

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24
Q

created the very first atomic theory

A

john dalton (1808)

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25
Q

english school teacher who performed many experiments on atoms

A

john dalton

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26
Q

viewed atoms as tiny, solid balls

A

john dalton

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27
Q

john dalton’s atomic theory

A
  • atoms are tiny, invisible particles
  • atoms of one element are all the same
  • atoms of diff elements are different
  • compounds form by combining atoms
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28
Q

dalton’s theory revisions

A
  • atoms aren’t indestructible; they consist of still smaller particles.
  • the atoms of one element may
    differ in mass
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29
Q

smaller particles that made up the atom

A

sub-atomic particles

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30
Q

not fundamental; divisible; positive

A

protons

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31
Q

made of two up quarks and one down quark

A

protons

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32
Q

not fundamental; divisible; negative

A

neutrons

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33
Q

made of one up quark and two down quarks

A

neutrons

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34
Q

fundamental; indivisible

A

electrons

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35
Q

still not known to consist of other particles

A

electrons

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36
Q

using his expertise in electromagnetic theory, he was able to determine the ratio of electron’s charge to its mass:

e- charge/m = − 𝟏.𝟕𝟔 𝐱 𝟏𝟎𝟖 𝐂/g

A

Sir Joseph John Thomson

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37
Q

oil-drop experiment

A

Robert Andrews Millikan

38
Q

mass of an electron

A

mass of an e- = (e-charge) ÷ (e-charge/mass)

39
Q

negatively charged particles

A

electrons

40
Q

-1 is the unit of negative charge

A

electrons

41
Q

value of the unit charge

A

electrons

42
Q

e = -1.60210 x 10-19 C

A

electrons

43
Q

has a mass of 9.109 x 10-28 g or 0.000549 amu

A

electrons

44
Q

positively charged particles

A

protons

45
Q

+1 is the unit of positive charge and
relative value

A

protons

46
Q

has a mass of 1.673 x 10-24 g or 1 amu

A

protons

47
Q

discovered electrons

A

JJ Thomson (1897)

48
Q

first scientist to show that the atom was made of even smaller things

A

JJ Thomson

49
Q

proposted the existence of a (+) particle

A

JJ Thomson

50
Q

his atomic model was known as the “raisin bun” model

A

JJ Thomson

51
Q

atoms are mostly made of (+) charged material, like dough in a bun; the (-) charged electrons are found inside the dough

A

raisin bun model by JJ Thomson

52
Q

gold foil experiment

A

rutherford and co.

53
Q

atom had a very dense (+) center; ____ called it a nucleus

A

rutherford

54
Q

mostly empty space

A

rutherford’s nuclear model

55
Q

has a small, positive nucleus containing protons

A

rutherford’s nuclear model

56
Q

negative electrons are scattered around it

A

rutherford’s nuclear model

57
Q

improved on Rutherford’s model

A

niel bohr (1913)

58
Q

proposed that electrons move around the nucleus in specific layers/shells

A

niel bohr

59
Q

every atom has a specific number of shells

A

niel bohr

60
Q

electrons move in definite orbits around the nucleus

A

bohr’s planetary model

61
Q

proposed by Erwin Schrödinger

A

schrodinger’s wave mechanical model

62
Q

electrons move like waves around the nucleus

A

schrodinger’s wave mechanical model

63
Q

atomic model that has electrons moving around the nucleus in a cloud

A

modern

64
Q

a modified wave mechanical model

A

born’s electron cloud model

65
Q

spherical cloud of varying density which shows where an electron is more or less likely to be

A

born’s electron cloud model

66
Q

discovered neutrons

A

james chadwick (1932)

67
Q

while working with rutherford, discovered particles that had no charge; he called them neutrons

A

james chadwick

68
Q

neutral, no electric charge

A

neutrons

69
Q

the other particle inside the nucleus aside from the protons that makes up the atomic mass

A

neutrons

70
Q

has a mass of 1.675 x 10-24 g or 1 amu

A

neutrons

71
Q

identity number

A

atomic number

72
Q

equal to the number of protons in the nucleus

A

atomic number

73
Q

equal to the number of electrons in the
neutral state

A

atomic number

74
Q

represented by capital letter “Z”

A

atomic number

75
Q

the sum of the number of neutrons and protons in an atomic nucleus

A

mass number

76
Q

represented by letter “A”

A

mass number

77
Q

the mass of an atom expressed in atomic mass units (µ)

A

atomic mass

78
Q

atoms that gain or lose electrons,
thereby forming charged particles

A

ions

79
Q

two types of ions

A

cations (+) and anions (-)

80
Q

formula for atomic number

A

Z = p

81
Q

formula for mass number

A

A = Z, A = p + n

82
Q

formula for neutrons

A

n = A - Z or p

83
Q

formula for e-

A

p if the electrical charge is 0 (neutral state)

84
Q

formula if the charge is + (cation)

A

p - charge = #e-

85
Q

formula if the charge is - (anion)

A

p + charge = #e-

86
Q

p + n =

A

atomic mass

87
Q

atoms are

A

neutral

88
Q

protons =

A

electrons

89
Q

do protons = atomic number?

A

yes

90
Q

what make up the identity of an atom?

A

number of protons

9 Chemistry (13 decks)

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