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1A Physical Science > Atomic Structure... > Flashcards

Atomic Structure... Flashcards

1
Q

element

A

substance that can’t be broken down into simpler substances

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2
Q

each element is made up of how many atoms

A

one

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3
Q

what makes each element different from each other

A

the number of protons

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4
Q

the periodic table lists

A

all of the elements currently known

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5
Q

relative masses of the 3 sub-atomic particles in an atom

A

electron 0/ proton 1/ neutron 1 amu

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6
Q

atom

A

smallest part of an element that still retains the uniqueness of that element

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7
Q

atoms are (size)

A

extremely small, a few 10 billionths of a meter

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8
Q

the atom consists of a ____ at the center

A

nucleus

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9
Q

what circles the nucleus in different orbits

A

electrons

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10
Q

all atoms consist of 2 main regions, what are they

A

nucleus, electron cloud

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11
Q

nucleus

A

small, dense, central part of an atom

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12
Q

the nucleus is ___ charged

A

positively charged

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13
Q

the nucleus makes up the entire __ of an atom

A

mass

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14
Q

electron cloud

A

the region in an atom surrounding the nucleus

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15
Q

all atoms are made up of 3 particles, they are

A

protons, neutrons, electrons

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16
Q

protons

A

positive, found in nucleus & with neutrons

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17
Q

neutrons

A

neutral, found in nucleus & with protons

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18
Q

electrons

A

negative, found in electron cloud

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19
Q

the positive charge of protons & negative charge of electrons create the ______ _____

A

electromagnetic force

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20
Q

what does the electromagnetic force do

A

bind the atoms together

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21
Q

the amount of protons & neutrons in an atom are

A

equal

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22
Q

the atom is electrically ____

A

neutral

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23
Q

theories

A

sum up hypothesis which explain why/how things happen that have been hold to show true with repeated testing

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24
Q

theories are not ____ but they are generally expected to be true

A

facts

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25
Q

laws

A

sum up a body of observations to explain what will happen in certain conditions ** without trying to explain why it will happen.

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26
Q

atomic theory

A

we can’t observe the structures of atoms, so indirect evidence has been used to develop models of the atom

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27
Q

dalton discovery

A

“Billard Ball” solid atoms are the building block of all matter.

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28
Q

dalton experiment

A

mixtures of gases to see what effect the individual gases making up the mixture had on the mixture as a whole

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29
Q

dalton new atomic theory

A

each type of atom is represented by a tiny solid sphere with a different mass, no internal structure

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30
Q

Thompson discovery

A

“Plum Pudding” electron is discovered

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31
Q

Thompson experiment

A

sealed gas tubes that had metal plates on each end. when connected to electrical source a beam formed. beam bent away from neg charged plate and towards the pos plate

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32
Q

thompson new atomic theory

A

an atom is a positively charged sphere which has negatively charged electrons spread evenly about its surface

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33
Q

rutherfords discovery

A

“Classical Solar System” atoms have a nucleus

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34
Q

Rutherfords experiment

A

sent a narrow beam of alpha particles through a thin sheet of gold

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35
Q

rutherfords new atomic theory

A

that there is a nucleus to an atom which contains positively charged protons & electrons circling the nucleus

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36
Q

bohr discovery

A

“shell” electrons travel in fixed orbits around the nucleus

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37
Q

bohr new atomic theory

A

electrons move with constant speed in fixed spherical orbits around the nucleus

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38
Q

current electron cloud model

A

“quantum mechanical” nucleus is surrounded by electron cloud

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39
Q

overall charge of all atoms

A

neutral

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40
Q

what makes carbon an element (opposed to a compound)

A

1 type of atom. It cannot be broken down simpler. A compound contains atoms of different elements.

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41
Q

How does the element carbon structurally differ from any other element

A

The number of protons is unique to carbon. There are 6.

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42
Q

mass number is not…

A

on the periodic table

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43
Q

how to calculate mass number

A

of protons + # of neutrons

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44
Q

this model was developed based on the evidence that the atom has a dense nucleus at the center

A

Rutherford

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45
Q

this model was developed based on the evidence that all matter was made of atoms, or solid spheres

A

Dalton

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46
Q

this model was developed based on the evidence that there is a negatively charged particle in an atom

A

Thompson

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47
Q

this model was developed based on the evidence that electrons travel in fixed orbits around the nucleus

A

Bohr

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48
Q

this model was developed based on the evidence that electrons are more likely to be located in certain regions more so than others

A

Electron Cloud

49
Q

every element has a different number of ____ which makes it unique

A

protons

50
Q

The periodic table organizes elements into ____ & ____-

A

families and periods

51
Q

families

A

vertical columns (up and down)

52
Q

periods

A

horizontal rows

53
Q

The top number on a periodic square

A

atomic number

54
Q

Letter abbreviation on periodic square

A

element symbol

55
Q

number on the bottom of a periodic square

A

atomic mass

56
Q

atomic number-

A

number of protons in an atom of that element, will also be the # of electrons

57
Q

element symbol-

A

1st letter always capitalized, 2nd lowercase

58
Q

atomic mass-

A

average mass of an elements atom.

59
Q

mass number-

A

mass of an individual isotope of an element (by adding protons and neutrons together AMU)

60
Q

AMU stands for

A

atomic mass units

61
Q

How to find number of neutrons

A

either
mass #-atomic # OR
rounded atomic mass - atomic #

62
Q

how to find most common mass #

A

round atomic mass

63
Q

what are both parts of this example: Hydrogen-1

A

name of element- mass number

64
Q

isotope

A

atoms of the same element that have different numbers of neutrons & mass numbers

65
Q

each proton and neutron add

A

one amu each

66
Q

2 ways to show an isotope

A

1- the name of the element- mass number

2- chemical symbol (letter) of the element with mass number on top & atomic number on bottom

67
Q

most elements have more than one ____

A

isotope

68
Q

how to calculate atomic mass

A

(# of 1st isotope x mass number of isotope given after dash) + (# of 2nd isotope x mass of isotope given after dash) / # of 1st isotope + # of 2nd isotope

69
Q

we know the most common isotope of blank is because

A

of calculating the average mass of the

mixture of its isotopes

70
Q

The bohr model of the atom is referred to as

A

the planetary model

71
Q

the bohr model is not the current model, but

A

its one to easily draw and use to show key characteristics of an atom

72
Q

in the bohr model the nucleus shows

A

the amounts of protons and neutrons P= N=

73
Q

1st orbital can hold how many electrons

A

2

74
Q

2nd & 3rd orbital can hold how many electrons

A

8 each

75
Q

the orbitals must be filled in

A

order, can’t add electrons to the 2nd orbital till there is 2 electrons on the first orbital

76
Q

how many elements of this element have this mass? (example)

A

none, no two elements are the same

77
Q

can this element have another atomic number? (example)

A

no, the amount of protons identify the element.

78
Q

charge of the electron cloud is

A

negative

79
Q

how do you name an isotope

A

ex. silicon-29

80
Q

what is the mass number of silicon-29

A

29

81
Q

why can the element pictured above have an isotope with a different mass number?

A

because there can be a different amount of neutrons

82
Q

most common isotope is the same as saying

A

the rounded atomic mass

83
Q

how do you know this is the most common isotope of an element?

A

averages are always closer to what there is more of

84
Q

the amount of ___ always stays the same, the amount of ___ can vary

A

protons, neutrons

85
Q

what does the atomic mass tell us about an element

A

the average mass of the mixture of its isotopes

86
Q

how many types of atoms make up an element

A

one

87
Q

what makes an element an element

A

elements are made up of one type of atom that can’t be broken down

88
Q

amount of protons make the elements

A

differ from each other

89
Q

what is a valence electron

A

electrons that are located on the outermost orbital of an atom

90
Q

Why do some elements not want to form bonds with anything else?

A

if its full it won’t be able to share electrons

91
Q

Which elements don’t want to form bonds and what do we call them

A

Nonmetals- Noble gasses

92
Q

why do some atoms gain or loose electrons

A

so they become more stable

93
Q

what do the dots on an electron dot diagram represent

A

valance electrons

94
Q

to find the energy level/orbitals of an atom you must

A

count from the highest square on the periodic table ( either hydrogen or helium) and count by one for each row until you get to the row of that element

95
Q

atoms want to be

A

stable

96
Q

to be stable atoms need to have

A

completely filled the outermost orbital

97
Q

ALL family 8 elements are ___ &

A

stable & do not react easily with other elements

98
Q

atoms that do not have their outer orbital filled completely want to

A

gain or lose electrons to become stable

99
Q

atoms that want to gain electrons

A

have 5,6 or 7 electrons on outermost energy level

100
Q

atoms that want to lose electrons

A

have 1,2,or 3 electrons on outermost energy level

101
Q

metalloids located

A

alongside stair step line

102
Q

metals located

A

to the left of stair step line

103
Q

non metals located

A

to the right of stair step line

104
Q

atomic radius increases from

A

the right & also down. (highest on the left, the lower down the element is the higher)

105
Q

valance electrons are identified by

A

the number on top of the table column. The column/family the element is in

106
Q

atomic radius is

A

the size of the atom

107
Q

reactivity

A

this is the tendency for an element to undergo a chemical change.

108
Q

reactivity on the periodic table- Highest reactivities are associated with what elements

A

elements that most want to gain or lose electrons

109
Q

metals reactivity tends to (R & L)

A

increase as you move from the right to the left. (highest at left side)

110
Q

metal reactivity tends to (Up & Down)

A

increase as you move down a column (lowest highest)

111
Q

non metals reactivity trends (R & L)

A

increase as you move from right to left (highest left side) as you move L-R more protons are present

112
Q

Non metals reactivity trends (Up & Down)

A

increases as you move up a column (Highest Highest)

113
Q

Elements that are non reactive at all

A

the noble gases (Family 8)

114
Q

what causes the general trends of atomic radii

A

more protons are present in the atoms nucleus

115
Q

what causes the general trends in reactivity

A

reactivity becomes larger because there is less distance between protons and outer electrons

116
Q

atomic radius increases

A

from right to left ; and down

117
Q

metal reactivity increases

A

from right to left; down

118
Q

electron dot diagram

A

diagram that are used to represent the structure of an tom, mostly focusing on valance electrons

1A Physical Science (4 decks)

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