QUIZ 3.2 Flashcards

1
Q

nucleus=

A

SMALL/DENSE/ POSITIVE

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2
Q

_____ orbit the nucleus,

A

ELECTRONS

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3
Q

atom =

A

EMPTY SPACE

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4
Q

_____ are orbiting around the
nucleus, accelerating, releasing energy.

A

ELECTRONS

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5
Q

electrons can only exist in

A

SHELLS

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6
Q

An electron can exist at

A

SPECIFIC DISTANCES FROM NUCLEUS

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7
Q

An electron _____be in between
_____levels

A

CANNOT
ENERGY

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8
Q

The _____is naturally attracted towards
the _____of the atom.

A

ELECTRON
NUCLEUS

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9
Q

electron absorbs energy=

A

HIGHER ENERGY LEVEL

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10
Q

If an electron is at a higher energy level, we
say that the electron is

A

EXCITED STATE

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11
Q

When an electron releases energy, it jumps
to a _____

A

LOWER ENERGY LEVEL/ GROUND STATE

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12
Q

energy enters the atom=

A

ELECTRON CAN ABSORB ENERGY BEXOMING EXCITED AND JUMP HIGHER ENERGY LEVELS

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13
Q

When the electron releases the
energy =

A

ELECTRON RETURNS TO LOWER ENERGY LEVELS

OTHER FORMS OF ELECTROMAGENETIC RADIATION BESIDE VISIBLE LIGHT CAN BE EMITTED

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14
Q

Each energy level can hold

A

CERTAIN NUMBER OF ELECTRON

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15
Q

The first level can hold

A

2

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16
Q

the
second can hold

A

8

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17
Q

and the third
can hold

A

18

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18
Q

no of e-

A

2N2

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19
Q

Inside each energy level, there are _____

A

SUBLEVELS

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20
Q

Inside the sublevels are _____

A

ORBITALS

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21
Q

Space around a nucleus where an
electron is likely to be found

A

ORBITALS

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22
Q

Orbitals are NOT _____.

A

ORBITS

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23
Q

Shape represents =

A

ELECTRON DENSITY NOT PATH

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24
Q

Each orbital can hold=

A

2 ELECTRONS

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25
When electrons occupy orbitals =
SPIN ON THEIR AXIS
26
If 2 electrons occupy an orbital =
SPIN OPPOSITE DIRECTIONS
27
Arrows are used to symbolize
E-
28
Electrons exist the in the
SPECIFIC ENERGY LEVELS ( SHELLS)
29
Inside the energy levels are
SUBLEVELS SPDF
30
Orbitals are NOT
ELECTRON PATHS
31
Energy Level – Energy sub level - orbital
A
32
In the ground state of an atom, electrons fill atomic orbitals of the _____ before occupying higher levels.
LOWEST ENERGY
33
_____ tells us that if we arrange the elements in order of increasing atomic number, we periodically encounter elements that have similar chemical and physical properties.
PERIODIC LAW
34
Arranged in ____ number
INCREASING ATOMIC NUMBER
35
columns =
GROUPS
36
rows =
PERIODS
37
Elements in a group
SIMILAR PROPERTIES
38
Group IA: Group 2A: Group 6A: Group 7A: Group 8A: Group B:
ALKALI METALS EARTH METALS CHALCOGENS HALOGENS NOBLE GASES TRANSITION METALS
39
57 – 71
LANTHANIDES
40
89 – 103
ACTINIDES
41
increases from top to bottom and decreases from left to right with respect to position in the periodic table.
METALLIC PROPERTY
42
Within a group, _____ increase from top to bottom as _____are added to shells farther from the nucleus.
ATOMIC RADII ELECTRONS
43
Atomic radii decrease from____within a given period
LEFT TO RIGHT
44
Down a group, the atomic radii increases because the =
NUMBER OF SHELL INCREASES
45
Across a period, the charge of the nucleus increases
PULLING ELECTRON CLOSER
46
_____of energy required to remove the most loosely bound electron from an isolated gaseous atom to form an ion with a 1+ charge.
IONIZATION ENERGY
47
Ionization energies measure how _____ electrons are bound to atoms.
TIGHTLY
48
_____ always requires energy to remove an electron from the attractive force of the nucleus.
IONIZATION
49
Low ionization energies indicate ease
REMOVAL ELECTRONS
50
_____ is the energy change that occurs when an electron is added to a gaseous atom
ELECTRON AFFINITY
51
Elements with very negative electron affinities _____
GAIN ELECTRONS EASILY TO FORM NEGATIVE IONS
52
_____ of an element is a measure of the relative tendency of an atom to attract electrons to itself when it is chemically combined with another atom.
EN ELECTRONEGATIVITY
53
F is the most _____
ELECTRONEGATIVITY
54
Noble gases are not ____
ELECTRONEGATIVE
55
same number proton different number of neutron
ISOTOPES
56
Atomic mass =
PROTON NEURTON
57
who asked " what makes up everything"
GREEKS
58
proposed idea that materials are composed of four elements fire/water/air/earth
ARISTOTLE
59
atomic theory of matter
JOHN DALTON ENGLISH CHEMIST METEOROLOGIST
60
law of conservation mass
ANTOINE LAVOISER
61
law of definite proportions
JOSEPH PROUST FRENCH CHEMIST
62
discovered negative electron
JONJOSEPH THOMSON
63
designed experiment to study alpha particle gold foil
ERNEST RUTHERFORD
64
danish physicist discovered electron in atom exist in specific region
NIELS BOHR
65
negatively charged ion
ANION
66
positively charged ion
CATION