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AP Chem > Chapter 7 > Flashcards

Chapter 7 Flashcards

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1
Q

electrons outside nucleus are attracted to the __ in the nucleus

A

protons

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2
Q

electrons propagate through space as an __ __

A

energy wave

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3
Q

electromagnetic radiation propagates through space as a __ moving at the speed of __

A

wavelight

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4
Q

1 nm = __ m

A

1 x 10^-9 m

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5
Q

The __ of electromagnetic radiation is directly proportional to the __ of the radiation

A

energyfrequency

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6
Q

Long wavelength = __ frequency = __ energyShort wavelength = __ frequency = __ energy

A

low, lowhigh, high

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7
Q

E = hv , E = energy in joules (__)

A

kg*m^2/s^2

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8
Q

As the electron moves toward the nucleus, the wavelength __

A

shortens

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9
Q

Shorter wavelength = __ energy = __ distance from the nucleus

A

highergreater

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10
Q

Electron transitions involve __ of definite amounts of __. This produces __ of light with definite __

A

jumpsenergybandswavelengths

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11
Q

Many elements give off characteristic __ which can be used to help identify them

A

light

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12
Q

Flame Tests: __ red/orange, __ orange, __ orange/yellow, __ magenta, __ violet, __ green, __ yellow/green

A

strontium, calcium, sodium, lithium, potassium, copper, barium

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13
Q

One cannot simultaneously determine both the position and momentum of an electron

A

Heisenberg Uncertainty Principle

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14
Q

More certain you are about where the electron is, the less certain you can be about where it is __ and vice versa

A

going

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15
Q

Denotes the probable distance of the electron from the nucleus

A

Electron energy level (shell)

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16
Q

Number of electrons that can fit in a shell (n)

A

2n^2

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17
Q

region within an energy level where there is a probability of finding an electron

A

orbital

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18
Q

the surface that contains 90% of the total electron probability

A

orbital shape

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19
Q

S-orbitalShape:# of orientations:# of max electrons:

A

Shape: spherical# of orientations: 1# of max electrons: 2

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20
Q

P-orbitalShape:# of orientations:# of max electrons:

A

Shape: dumbbell# of orientations: 3# of max electrons: 6

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21
Q

D-orbitalShape:# of orientations:# of max electrons:

A

Shape: double dumbbell# of orientations: 5# of max electrons: 10

22
Q

F-orbitalShape:# of orientations:# of max electrons:

A

Shape: complex# of orientations: 7# of max electrons: 14

23
Q

Number of electrons per main energy level:n=1:n=2:n=3:n=4:

A

n=1: 2n=2: 8n=3: 18n=4: 32

24
Q

2 electrons occupying the same orbital must have opposite spins

A

Pauli exclusion principle

25
Q

E(ns) __ E(np) __ E(nd) __ E(nf)

A

E(ns)

26
Q

Most chemically reactive metals are found on the __ __ hand side of the table, where the __ __ is smallest

A

lower leftionization energy

27
Q

Most chemically reactive nonmetals are found on the __ __ hand side of the table, where the __ __ is largest

A

upper rightionization energy

28
Q

Half the distance between nuclei in covalently bonded diatomic molecule

A

atomic radius

29
Q

Atomic radius __ across a period. Increased __ __ __ due to __ shielding

A

decreaseseffective nuclear chargedecreased

30
Q

Atomic radius __ down a group. Each row on the periodic table adds an __ __ to the atom

A

increasesenergy level

31
Q

The energy required to remove an electron from an atom. Increases for successive electrons taken from the same atom

A

Ionization energy

32
Q

Ionization energy tends to __ across a period. Electrons in the same quantum level don’t __ as effectively as electrons in inner level

A

increaseshield

33
Q

Ionization energy tends to __ down a group. Outer electrons are farther from the nucleus and __ to remove

A

decreaseeasier

34
Q

The energy change associated with the addition of an electron

A

Electron affinity

35
Q

Electron affinity tends to __ across a period

A

increase

36
Q

Electron affinity tends to __ down a group. Electrons farther from the nucleus experience __ nuclear attraction

A

decreaseless

37
Q

A measure of the ability of an atom in a chemical compound to attract electrons

A

electronegativity

38
Q

Electronegativity tends to __ across a period. As radius decreases, electrons get __ to the bonding atom’s nucleus

A

increasecloser

39
Q

Electronegativity tends to __ down a group or __ __ __. As radius increases, electrons are __ from the bonding atom’s nucleus

A

decreaseremain the samefarther

40
Q

__ radius decrease across a period, __ are bigger to the left and become smaller

A

cationsanions

41
Q

Positively charged ions formed when an atom of a metal loses one or more electrons. __ than the corresponding atom

A

cationssmaller

42
Q

Negatively charged ions formed when non metallic atoms gain one or or more electrons. __ than the corresponding atom

A

anionslarger

43
Q

Attraction that occurs between oppositely charged particles. (__ in nucleus to __ surrounding the nucleus)

A

Coulombic attractionprotonselectrons

44
Q

Net positive charge “felt” by the valence electron. Takes into account attractive forces felt b/w the protons and electrons, as well as the repulsive forces felt b/w valence electrons and core electrons

A

Effective nuclear charge

45
Q

Electrons intervening b/w nucleus and valence electrons are said to __ the valence electrons from the nucleus so that the valence electrons don’e experience the full __ __ of the positive nuclear charge

A

shieldattractive pull

46
Q

Coulombic attraction __ across a period. There are the same # of __ __, but there are more __ resulting in a greater attraction of valence electrons to the nucleus

A

increasesenergy levelsprotons

47
Q

Coulombic attraction __ down a group. There are more __ __, more __ between valence electrons resulting in a weaker attraction of outer electrons to the nucleus

A

decreasesenergy levelsdistance

48
Q

__ __ is when it loses electrons and creates a positive ion

A

ionization energy

49
Q

Most half-filled orbitals, most unpaired electrons

A

paramagnetic

50
Q

Most protons, most effective nuclear charge

A

isoelectronic

51
Q

List the electromagnetic radiation from the longest to the shortest wavelengths (7)

A

Radio waves, Microwaves, Infrared, Visible, Ultraviolet, X-rays, Gamma rays

AP Chem (11 decks)

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