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SL Chemistry > Unit 3: Electrons And Periodicity > Flashcards

Unit 3: Electrons And Periodicity Flashcards

0
Q

Speed of Light Measurement

A

3.00xE8 m/s

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1
Q

Light

A

A kind of ELECTROMAGNETIC RADIATION.

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2
Q

Trough

A

The bottom curve of a wave

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3
Q

Crest

A

Upper curve of a wave

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4
Q

Wavelength

A

Shortest distance between equivalent points on a continuous wave
(Represented by an upside down y)

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5
Q

Frequency

A

Number of Waves that pass a given point per second

CYCLES/SEC or HERTZ (Hz)

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6
Q

Frequency and Wavelength…..

A

Are inversely related, when frequency goes up wavelength is shorter

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7
Q

Electromagnetic Spectrum Order…

A 
Radio Waves 
Microwaves 
Infrared 
Visible Light
Ultraviolet 
X-Rays 
Gamma Rays
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8
Q

Low Energy has ——– Frequency and ——- Wavelengths

A

Low Frequency and Long Wavelengths

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9
Q

High Energy has ——- Frequency and ——- Wavelengths

A

High Frequency and Shorter Wavelengths

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10
Q

Max Planck

A

German Physicist

Discovered Quantum, photons, and relationships between frequency and energy

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11
Q

Quanta

A

Gain or lose of energy in small specific amounts.(matter)

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12
Q

Photons

A

Tiny particles of electromagnetic radiation or BUNDLES of energy with NO MASS
Carries a quantum of energy

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13
Q

Energy of Quantum is directly related to…….

A

The frequency of the empires radiation

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14
Q

Frequency of light increases…..

A

Energy of a photon increases

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15
Q

Photoelectric Effect

A

Proposed by Einstein.

Electrons are emitted from a metals surface when light of a certain frequency shines on the surface

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16
Q

The further from the nucleus an energy level is…..

A

…. The higher the energy (ring or ladders)

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17
Q

Bohr

A

Created the Bohr Model of the Atom which describes electrons in different orbitals and the movements involved.

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18
Q

Ground State

A

Lowest allowable energy state of an atom

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19
Q

Excited State

A

When an atom gains energy. Can drop from higher energy orbit to lower.

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20
Q

Transition of an electron from high to low or low to high emits a …….

A

Photon that corresponds to the difference between the energy levels associated with the two orbits

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21
Q

Line Spectra

A

When an element gives off it’s own color, it can be identified through the line spectrum

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23
Q

Emission

A

The spectrum of piggy released from excited atoms of an element

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24
Q

Principal Quantum

A

Main Energy Levels (1,2,3,4). Contains Subshells

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25
Angular Momentum
Shape of Orbital
26
Magnetic Quantum
Orientation
27
Spin Quantum
States of Electrons
28
Electron Cloud
Space around the nucleus where electrons are expected to be found
29
Atomic Orbital
3-Dimensional region around the nucleus that describes the probable location of an electron
30
Subshells
S - 2 Electrons P - 6 Electrons D - 10 Electrons F - 14 Electrons
31
S Orbital Shape
1 Spherical Shape and @ Energy Level 1
32
P Orbital Shape
3 Dumbbell Shaped (3) and @ Energy Level 2
33
D Orbital Shape
5 Different Shapes and @ Energy Level 3
34
F Orbital Shape
7 Different Shapes and @ Energy Level 4
35
Electron Configurations
``` Represents the way electrons are arranged in atoms Order: 1. Energy Level (1,2,3,4) 2. Sublevel/Orbital (S,P,D,F) 3. # of Electrons ```
36
Aufbau Principle
Electrons enter the LOWEST energy first. Causes difficulties because of overlaps of orbitals
37
Pauli Exclusion Principle
At most there can only be 2 Electrons per orbital and have opposite spins otherwise they would repel
38
Hund's Rule
When electrons occupy orbitals of equal energy, they don't pair up with an electron yet, they get their own space and then pair up.
39
Valence Electrons
Electrons in the Outermost energy level
40
Orbital Notation
The longer way to write Electron Configuration 1. Energy Level (1,2,3,4) 2. Orientation (Arrows) 3. # of Electrons 4. Spin
41
Dmitri Mendellev
Russian Chemist and "Father of Periodic Table" | Studied properties of elements and realized that properties repeated in a pattern.
42
Periodicity
Tendency to repeat at regular intervals
43
Henry Moseley
"Father of Modern Periodic Table" Discovered order or protons and what it meant.
44
Periodic Law
Physical and Chemical Properties of elements repeat in a regular pattern when they are arranged in order of increasing atomic number.
45
Period/Series
Elements in the Row
46
Groups/Family
Elements in Column
47
Representative Elements
Elements in Group A
48
Transition Elements
Elements in Group B
49
Inner Transition Elements
Two Rows of elements at the bottom
50
Alkali Metals
Elements in Group 1A. 1 Valence Electron and Loses 1 valence Electron
51
Alkaline Earth Metals
Elements in Group 2A. 2 Velance Electrons and loses 2 valence electrons
52
Boron Group
Elements in Group 3A. 3 Valance Electrons and loses 3 valence electrons
53
Carbon Group
Elements in Group 4A. 4 Valence Electrons and loses or gains valence electrons
54
Nitrogen Group
Elements in Group 5A. 5 Valence Electrons. Gains 3 Electrons
55
Oxygen Group
Elements in Group 6A. 6 Valence Electrons and gains 2 Valence Electrons
56
Halogens
Elements in Group 7A. 7 Valence Electrons and gains 1 Valence Electron
57
Noble Gases
Elements in Group 8A. 8 Valence Electrons and DO NOT lose or gain Valence Electrons
58
Reactivity
Ability to react with another substance
59
Metalloids
Lies between the border between metals and nonmetals. Same chemical and physical properties of other nonmetals.
60
Semiconductors
An Element that does not conduct electricity as metal
61
Atomic Radius
The Volume of an atom measured from nucleus to outside
62
Atomic Size is influenced by.....
Energy Levels | Charge in Nucleus
63
Anion
A negatively charged ion (gaining of ions)
64
Cation
Positively charged ion (loss of electrons)
65
Ionization Energy
The amount of energy required to completely remove an atom from a gaseous atom
66
Electronegativity
Tendency for an atom to attract electrons to itself when chemically combined with another element

SL Chemistry (18 decks)

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