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Honors Chemistry > Unit 3 > Flashcards

Unit 3 Flashcards

1
Q

Properties of Electromagnetic Waves

A

Wavelength
Frequency
Energy

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2
Q

Frequency Measured In

A

Nu

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3
Q

Electromagnetic Radiation

A

Form of energy that exhibits wavelike behaviour as it travels through space

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4
Q

Electromagnetic Spectrum

A

Arrangement of all electromagnetic waves by decreasing wavelength and increasing frequency

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5
Q

Electromagnetic Spectrum Order

A

Gamma
X-ray
Ultraviolet
Visible light
Infrared
Microwave
TV radio
AM radio
Long radio

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6
Q

Visible Light Amounts

A

Wavelength 1.0x10^-7 m
Frequency 1.0x10^14 Hz
Energy 1.0x10^-19 J

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7
Q

Quanta

A

Light does not produce energy continiously, but in packets called quanta

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8
Q

Quantum

A

Minimum amount of energy lost or gained by an atom due to its energy levels

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9
Q

Quantized Energy

A

Multiples of quanta

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10
Q

Energy Equation

A

E=hv

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11
Q

Planck’s Constant

A

6.626x10^-34 J*s

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12
Q

Photon

A

Particle of electromagnetic radiation Zero mass
Carrying a quantum of energy
Moves like waves

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13
Q

Line Emission Spectrum

A

Bands of light

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14
Q

Continiuous Spectra

A

White light that continuously emits lines of all colors

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15
Q

Line Emission Spectra

A

Only certain lines of color are seen

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16
Q

Four Arrangements of Electrons

A

Principle energy level
Sublevel
Orbital
Electrons spin

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17
Q

Sublevel S

A

Spherical shape
Holds 2 electrons

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18
Q

Sublevel P

A

Dumbell shape
Three P orbitals in 1 P sublevel
Holds 6 electrons

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19
Q

Sublevel D

A

Clover shape
Five D orbitals in 1 D sublevel
Holds 10 electrons

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20
Q

Sublevel F

A

Flower shape
Seven F orbitals in 1 F sublevel
Holds 14 electrons

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21
Q

Orbitals

A

Different orientations of shapes within a sublevel

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22
Q

Rules to Writing Electron Configurations

A

Aufbau
Pauli
Hund

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23
Q

Aufbau’s Principle

A

Electrons will occupy the lowest energy first

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24
Q

Pauli’s Exclusion Principle

A

A maximum of 2 electrons can fill an orbital if they have opposite spins

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25
Q

Hund’s Rule

A

Electrons will fill equal level orbitals until each has one before doubling up
All electrons have the same spin in each individually filled orbital

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26
Q

Excpetions

A

Column 11 and 6
Move S to D to make stable

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27
Q

D Doesn’t Count As

A

Valence electron

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28
Q

Coefficient on Last Sublevel

A

Energy level

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29
Q

Highest Sublevel

A

Block

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30
Q

Isoelectronic Series

A

Ions with the same electron configuration

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31
Q

Dmitri Mendeleev

A

Organized periodic table by atomic mass and similar row properties

32
Q

Henry Moseley

A

Rearranged elements by increasing atomic number

33
Q

Periodic Law

A

Physical and chemical properties of elements are periodic functions of their atomic number

34
Q

Length of Period

A

Determined by number of electrons that can occupy the sublevels filled in that row

35
Q

Elements in Same Group

A

Share properties
Share same number of valences

36
Q

Why Same Group Elements Have Similar Properties

A

Lose or gain same number of electrons when forming ions

37
Q

Metals

A

Elements containing atoms that readily lose electrons to form ions
Cations

38
Q

Chemical Metal Properties

A

Few electrons in valence level
Loses electrons readily
Positive charge
Forms cations

39
Q

Physical Metal Properties

A

Ductile
Malleable
High tensile strength
Good conductors
Luster
Forms alloys
Mostly solid at room temperature

40
Q

Alkai Metals

A

Always have one valence electron
Never found purely as too reactive

41
Q

Alkai Metals IA

A

Very reactive
Most reactive group of metals
Soft
Silvery

42
Q

Phenomenon

A

Alkai metlas plus water

43
Q

Alkaline Earth Metals IIA

A

Two valence electrons
Less reactive than alkali
Still not found pure
Alkaline means basic

44
Q

Transition Metals

A

D block elements
B groups
Typical metallic properties

45
Q

Lanthanides

A

Rare Earth metals
Silver
Tarnish in oxygen

46
Q

Actinides

A

Radioactive

47
Q

Nonmetals

A

Elements containing atoms that readily gain electrons to form negatuve ions
Anions

48
Q

Chemical Nonmetal Properties

A

Almost full or full valence energy level
Tend to gain electrons
Negative charge
Form anions

49
Q

Physical Nonmetal Properties

A

Not ductile
Not malleable
Bad conductors
Brittle
Mostly solid
Some are gases at room temperature

50
Q

Halogens VIIA

A

Seven valence electrons
Most reactive nonmetals group
Only found in pure form as diatomic

51
Q

Noble Gases VIIIA

A

Eight valence electrons
Colorless
Odorless
Chemically unreactive
Only found purely in nature

52
Q

Metalloids

A

In between metals and nonmetals

53
Q

Chemical Metalloid Properties

A

Form anions or cations depend on environment
Properties of both metals nonmetals

54
Q

Physical Metalloid Properties

A

Semiconductors
Some have metallic luster
Semiconductors of electricity
Some are gases at room temperature

55
Q

Periodic Trends Influenced By

A

Shielding
Charge on nucleus
Distance of electrons from nucleus

56
Q

Shielding Cause and Effects

A

Inner electrons repel outer blocks nuclear effects
Nucleus hold is weak causes electrons to be easier to remove

57
Q

Atomic Radius Cause and Effects

A

Increased charge attracts electrons inward
Energy level added makes it further from nucleus

58
Q

Ionic Radius Cause and Effects

A

Increased positive charge pulls electrons inward
More electrons than protons increases repulsive forces

59
Q

Ionization Energy

A

Energy required to remove an electron from an atom or how easily it becomes a cation

60
Q

Ionization Energy Cause and Effects

A

Atomic radius decreases causes valence electron to be closer
Valence electron is closer causes it to be held more tightly

61
Q

Electronegativity

A

Measure of the ability of an atom in a chemical compound to attract electrons from another atom or how easily it becomes and anion

62
Q

Electronegativity Cause and Effects

A

Positive nuclear charge causes stronger electron pull
Valence electrons further from nucleas causes it to be difficult to pull more in

63
Q

Nuclear Charge Down The Group and Across The Period

A

Increases

64
Q

Periodic Trends

A

Increasing nuclear charge and number of protons but same energy level

65
Q

Group Trends

A

Increasing shielding and number of energy level

66
Q

Reactivity Cause and Effects

A

Increase in shielding causes reactivity to decrease
Increase in shielding causes more orbits
More orbits causes less attraction

67
Q

Valence Electron Pattern

A

Increase across period
Remain same down a group

68
Q

Atomic Radius Pattern

A

Peaks on left and moves down then peaks again

69
Q

Metals VS Nonmetals Reaction

A

Lose VS gain electrons

70
Q

Electron Affinity

A

The amount of energy released when a neutral gaseous atom gains an electron

71
Q

Electron Affinity Cause

A

Greater nuclear charge releases more energy
Smaller valence shells means higher energy release

72
Q

Three Factors That Affect Electron Affinity

A

Nuclear charge
Atomic radius
Electron configuration

73
Q

Electron Affinity Pattern

A

Increase across period
Decrease down the group

74
Q

Diatomic Elements

A
75
Q

Metallic Character Cause and Effects

A

Nuclear charge increases from left to right
Electrons are pulled closer inward
Atom has more difficult time losing electrons
Increases metallic character

Honors Chemistry (9 decks)

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