Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Honors Chemistry > Unit 3 > Flashcards

Unit 3 Flashcards

1
Q

Properties of Electromagnetic Waves

A

Wavelength
Frequency
Energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Frequency Measured In

A

Nu

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Electromagnetic Radiation

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Electromagnetic Spectrum

A

Arrangement of all electromagnetic waves by decreasing wavelength and increasing frequency

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Electromagnetic Spectrum Order

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Visible Light Amounts

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Quanta

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Quantum

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Quantized Energy

A

Multiples of quanta

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Energy Equation

A

E=hv

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Planck’s Constant

A

6.626x10^-34 J*s

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Photon

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Line Emission Spectrum

A

Bands of light

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Continiuous Spectra

A

White light that continuously emits lines of all colors

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Line Emission Spectra

A

Only certain lines of color are seen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Four Arrangements of Electrons

A

Principle energy level
Sublevel
Orbital
Electrons spin

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Sublevel S

A

Spherical shape
Holds 2 electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Sublevel P

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Sublevel D

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Sublevel F

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Orbitals

A

Different orientations of shapes within a sublevel

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Rules to Writing Electron Configurations

A

Aufbau
Pauli
Hund

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Aufbau’s Principle

A

Electrons will occupy the lowest energy first

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Pauli’s Exclusion Principle

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Hund's Rule
Electrons will fill equal level orbitals until each has one before doubling up All electrons have the same spin in each individually filled orbital
26
Excpetions
Column 11 and 6 Move S to D to make stable
27
D Doesn't Count As
Valence electron
28
Coefficient on Last Sublevel
Energy level
29
Highest Sublevel
Block
30
Isoelectronic Series
Ions with the same electron configuration
31
Dmitri Mendeleev
Organized periodic table by atomic mass and similar row properties
32
Henry Moseley
Rearranged elements by increasing atomic number
33
Periodic Law
Physical and chemical properties of elements are periodic functions of their atomic number
34
Length of Period
Determined by number of electrons that can occupy the sublevels filled in that row
35
Elements in Same Group
Share properties Share same number of valences
36
Why Same Group Elements Have Similar Properties
Lose or gain same number of electrons when forming ions
37
Metals
Elements containing atoms that readily lose electrons to form ions Cations
38
Chemical Metal Properties
Few electrons in valence level Loses electrons readily Positive charge Forms cations
39
Physical Metal Properties
Ductile Malleable High tensile strength Good conductors Luster Forms alloys Mostly solid at room temperature
40
Alkai Metals
Always have one valence electron Never found purely as too reactive
41
Alkai Metals IA
Very reactive Most reactive group of metals Soft Silvery
42
Phenomenon
Alkai metlas plus water
43
Alkaline Earth Metals IIA
Two valence electrons Less reactive than alkali Still not found pure Alkaline means basic
44
Transition Metals
D block elements B groups Typical metallic properties
45
Lanthanides
Rare Earth metals Silver Tarnish in oxygen
46
Actinides
Radioactive
47
Nonmetals
Elements containing atoms that readily gain electrons to form negatuve ions Anions
48
Chemical Nonmetal Properties
Almost full or full valence energy level Tend to gain electrons Negative charge Form anions
49
Physical Nonmetal Properties
Not ductile Not malleable Bad conductors Brittle Mostly solid Some are gases at room temperature
50
Halogens VIIA
Seven valence electrons Most reactive nonmetals group Only found in pure form as diatomic
51
Noble Gases VIIIA
Eight valence electrons Colorless Odorless Chemically unreactive Only found purely in nature
52
Metalloids
In between metals and nonmetals
53
Chemical Metalloid Properties
Form anions or cations depend on environment Properties of both metals nonmetals
54
Physical Metalloid Properties
Semiconductors Some have metallic luster Semiconductors of electricity Some are gases at room temperature
55
Periodic Trends Influenced By
Shielding Charge on nucleus Distance of electrons from nucleus
56
Shielding Cause and Effects
Inner electrons repel outer blocks nuclear effects Nucleus hold is weak causes electrons to be easier to remove
57
Atomic Radius Cause and Effects
Increased charge attracts electrons inward Energy level added makes it further from nucleus
58
Ionic Radius Cause and Effects
Increased positive charge pulls electrons inward More electrons than protons increases repulsive forces
59
Ionization Energy
Energy required to remove an electron from an atom or how easily it becomes a cation
60
Ionization Energy Cause and Effects
Atomic radius decreases causes valence electron to be closer Valence electron is closer causes it to be held more tightly
61
Electronegativity
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
Electronegativity Cause and Effects
Positive nuclear charge causes stronger electron pull Valence electrons further from nucleas causes it to be difficult to pull more in
63
Nuclear Charge Down The Group and Across The Period
Increases
64
Periodic Trends
Increasing nuclear charge and number of protons but same energy level
65
Group Trends
Increasing shielding and number of energy level
66
Reactivity Cause and Effects
Increase in shielding causes reactivity to decrease Increase in shielding causes more orbits More orbits causes less attraction
67
Valence Electron Pattern
Increase across period Remain same down a group
68
Atomic Radius Pattern
Peaks on left and moves down then peaks again
69
Metals VS Nonmetals Reaction
Lose VS gain electrons
70
Electron Affinity
The amount of energy released when a neutral gaseous atom gains an electron
71
Electron Affinity Cause
Greater nuclear charge releases more energy Smaller valence shells means higher energy release
72
Three Factors That Affect Electron Affinity
Nuclear charge Atomic radius Electron configuration
73
Electron Affinity Pattern
Increase across period Decrease down the group
74
Diatomic Elements
75
Metallic Character Cause and Effects
Nuclear charge increases from left to right Electrons are pulled closer inward Atom has more difficult time losing electrons Increases metallic character

Honors Chemistry (17 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions