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SL Chemistry > Unit 3: Electrons And Periodicity > Flashcards

Unit 3: Electrons And Periodicity Flashcards

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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
Q

Angular Momentum

A

Shape of Orbital

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26
Q

Magnetic Quantum

A

Orientation

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27
Q

Spin Quantum

A

States of Electrons

28
Q

Electron Cloud

A

Space around the nucleus where electrons are expected to be found

29
Q

Atomic Orbital

A

3-Dimensional region around the nucleus that describes the probable location of an electron

30
Q

Subshells

A

S - 2 Electrons
P - 6 Electrons
D - 10 Electrons
F - 14 Electrons

31
Q

S Orbital Shape

A

1 Spherical Shape and @ Energy Level 1

32
Q

P Orbital Shape

A

3 Dumbbell Shaped (3) and @ Energy Level 2

33
Q

D Orbital Shape

A

5 Different Shapes and @ Energy Level 3

34
Q

F Orbital Shape

A

7 Different Shapes and @ Energy Level 4

35
Q

Electron Configurations

A 
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
Q

Aufbau Principle

A

Electrons enter the LOWEST energy first. Causes difficulties because of overlaps of orbitals

37
Q

Pauli Exclusion Principle

A

At most there can only be 2 Electrons per orbital and have opposite spins otherwise they would repel

38
Q

Hund’s Rule

A

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
Q

Valence Electrons

A

Electrons in the Outermost energy level

40
Q

Orbital Notation

A

The longer way to write Electron Configuration

  1. Energy Level (1,2,3,4)
  2. Orientation (Arrows)
  3. # of Electrons
  4. Spin
41
Q

Dmitri Mendellev

A

Russian Chemist and “Father of Periodic Table”

Studied properties of elements and realized that properties repeated in a pattern.

42
Q

Periodicity

A

Tendency to repeat at regular intervals

43
Q

Henry Moseley

A

“Father of Modern Periodic Table” Discovered order or protons and what it meant.

44
Q

Periodic Law

A

Physical and Chemical Properties of elements repeat in a regular pattern when they are arranged in order of increasing atomic number.

45
Q

Period/Series

A

Elements in the Row

46
Q

Groups/Family

A

Elements in Column

47
Q

Representative Elements

A

Elements in Group A

48
Q

Transition Elements

A

Elements in Group B

49
Q

Inner Transition Elements

A

Two Rows of elements at the bottom

50
Q

Alkali Metals

A

Elements in Group 1A. 1 Valence Electron and Loses 1 valence Electron

51
Q

Alkaline Earth Metals

A

Elements in Group 2A. 2 Velance Electrons and loses 2 valence electrons

52
Q

Boron Group

A

Elements in Group 3A. 3 Valance Electrons and loses 3 valence electrons

53
Q

Carbon Group

A

Elements in Group 4A. 4 Valence Electrons and loses or gains valence electrons

54
Q

Nitrogen Group

A

Elements in Group 5A. 5 Valence Electrons. Gains 3 Electrons

55
Q

Oxygen Group

A

Elements in Group 6A. 6 Valence Electrons and gains 2 Valence Electrons

56
Q

Halogens

A

Elements in Group 7A. 7 Valence Electrons and gains 1 Valence Electron

57
Q

Noble Gases

A

Elements in Group 8A. 8 Valence Electrons and DO NOT lose or gain Valence Electrons

58
Q

Reactivity

A

Ability to react with another substance

59
Q

Metalloids

A

Lies between the border between metals and nonmetals. Same chemical and physical properties of other nonmetals.

60
Q

Semiconductors

A

An Element that does not conduct electricity as metal

61
Q

Atomic Radius

A

The Volume of an atom measured from nucleus to outside

62
Q

Atomic Size is influenced by…..

A

Energy Levels

Charge in Nucleus

63
Q

Anion

A

A negatively charged ion (gaining of ions)

64
Q

Cation

A

Positively charged ion (loss of electrons)

65
Q

Ionization Energy

A

The amount of energy required to completely remove an atom from a gaseous atom

66
Q

Electronegativity

A

Tendency for an atom to attract electrons to itself when chemically combined with another element

SL Chemistry (18 decks)

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