Chapter 7 Electron Structure Of The Atom

Front 1

Energy that travels thru space at the speed of light as oscillating waves

Back 1

Electromagnetic radiation

Front 2

Number of wave cycles passing a stationary point in one second

Back 2

Hertz

Front 3

Amount of energy required to remove a valence electron from an atom or ion in the gaseous state

Back 3

Ionization energy

Front 4

A rule stating that electrons are distributed in orbitals of the same energy in such a way as to give the maximum number of unpaired electrons

Back 4

Hund

Front 5

A description of the distribution of electrons in an atom’s sublevels

Back 5

Electron configuration

Front 6

An inner electron that is not a valence electron

Back 6

Core electron

Front 7

A region in space where an electron is likely to be found

Back 7

Orbital

Front 8

A spectrum that consists of all the wavelengths of visible light

Back 8

Visible region of the electromagnetic spectrum

Front 9

Having the same number of electrons

Back 9

Isoelectric

Front 10

The distance between 2 corresponding points on a wave

Back 10

Wavelength

Front 11

The smallest packet of energy of a specific type of electromagnetic radiation

Back 11

Photon

Front 12

A measure of the size of an atom measured from the nucleus to the outer edge of the atom

Back 12

Atomic radius

Front 13

A rule stating that a maximum of 2 electrons can occupy an orbital and that the electrons must have opposite spin

Back 13

Pauli exclusion principle

Front 14

An electron that occupies the highest principle energy level

Back 14

Valence electron

Front 15

The lowest energy electron configuration

Back 15

Ground state

Front 16

An energy level consisting of orbitals of the same type and energy

Back 16

Valence level

Front 17

A spectrum of an element or molecule which uniquely identifies it

Back 17

Line spectrum

Front 18

Having only specific allowed values

Back 18

Quantized

Front 19

List 3 types of electromagnetic radiation that have longer wavelengths than visible light

Back 19

Microwave, Infrared, radio

Front 20

The number of levels in the S orbital

Back 20

One

Front 21

The shape of the P orbital and the number of orbitals in the P sublevel

Back 21

Three shaped like a dumbell

Front 22

Rule which states that electrons fill orbitals starting with the lowest energy orbitals first

Back 22

Aufbau principle

Hint 22

To build up

Front 23

The lowest energy state of an atom

Back 23

Ground state

Front 24

The maximum number of electrons found in any main energy level can be determined by the formula 2n^2 where n is the?

Back 24

Principle energy level

Front 25

A region of space in which one or two electrons are found

Back 25

Orbital

Front 26

For n = 2 the total number of electrons would be?

Back 26

8

Hint 26

2 (2^2)

Front 27

Symbols by which sub levels are indicated

Back 27

S P D F

Front 28

What does the symbol 4S^2 represent?

Back 28

Energy level 4 (period 4)

Sublevel S

number of electrons (2)

Front 29

Sub level that contains 5 orbitals

Back 29

D Sublevel

Front 30

Electron configuration for iron (Fe)

Back 30

1s2 2s2 2p6 3s2 3p6 4s2 3d6

Front 31

Elements that tend to form mono atomic ions by gaining one or more electrons

Back 31

Non metals

Front 32

Which subatomic particles are involved in the production of light?

Back 32

Electrons

Front 33

The lowest energy state of an atom

Back 33

Ground state

Front 34

A particle of light is called a

Back 34

Photon

Front 35

What type of energy is light?

Back 35

Electromagnetic radiation

Radiant

Front 36

Using ROYGBIV, which has the longest wavelength?

Back 36

Red

Front 37

Using ROYGBIV which has the highest energy?

Back 37

Violet

Front 38

Using ROYGBIV which has the lowest frequency?

Back 38

Red

Front 39

Visible spectrum wavelengths range from violet nm? To red nanometers?

Back 39

400 to 750

Front 40

What is the atomic number for 1s2 2s2 2p6 3s2 3p6 4s2

Back 40

20

Hint 40

Add the superscripts

Front 41

Delta energy =

Back 41

E(final) - E(initial)

Front 42

Which transition has the highest energy?

4 -> 2

4 -> 1

1 -> 4

2 -> 4

Back 42

4-1 because 4 minus one is three. Also we are measuring transition energy where the electron is falling from a higher level to a lower level

Front 43

When an electron occupies an energy level higher than the lowest energy level it is in what state?

Back 43

Excited state

Front 44

Using ROYGBIV, which has the longest wavelength?

Back 44

Red

Front 45

Subshell

Back 45

All the orbitals of one type within a shell

Front 46

Symbols by which sub levels are kndicated

Back 46

S P D F

Front 47

Visible spectrum wavelengths range from violet nm? To red nanometers?

Back 47

400(violet)

750 (red)

Front 48

Sub level that contains 5 orbitals

Back 48

P Sublevel

Front 49

Delta energy = E(final) - E(initial)

Back 49

Back (Definition)

Front 50

Elements that tend to form mono atomic ions by gaining one or more electrons

Back 50

Non metals

Front 51

Periodic trend of atomic radii

Back 51

Top to bottom increasing. Right to left increasing. Runs counterclockwise.

Front 52

Ionization energy trend

Back 52

Bottom to top increasing

Left to right increasing.

Runs clockwise

Front 53

What is the abbreviated electron config for Al3+ ion

Back 53

Al 3+ = [Ne]3s2 3p1

Minus 3 electrons

Becomes [Ne]

Front 54

Which element has greater ionization energy, F or C

Back 54

F because it is further to the right of carbon and it also has a higher electronegativity

Front 55

Ionization energy increases from ? To ? And ? To ?

Back 55

Left to right and bottom to top

Front 56

The size of an atom is described in terms of its ?

Back 56

Atomic radius

Front 57

The lithium ion in terms of atomic size is smaller/larger than the lithium atom?

Back 57

Smaller because it loses an electron and contracts

Front 58

The fluorine ion becomes smaller/larger than the fluorine atom?

Back 58

Larger because fluorine gains an electron thus it expands

Front 59

What is the speed of light in a vacuum?

Back 59

3.00x10^8 meters per second

Front 60

For any isoelectronic series as the number of ___ increases the ion size ___

Back 60

Protons

Decreases

Front 61

Ionization energy trend

Back 61

Bottom to top increasing

Left to right in reading.

Runs clockwise

Front 62

Ionization energy factors

Back 62

Charge

Distance (of electron from nucleus)

Shielding (valence electrons)

More protons

Front 63

Valence level (shell)

Back 63

The last occupied principle energy level

Front 64

Order atoms by their size

Back 64

Periodic trend is counterclockwise. Starting from lower left largest to upper right smaller. Also each group runs smallest from top of group to largest at bottom of group

Front 65

S block elements are groups __ And___. They are known as ___metals and ____metals

Back 65

1 and 2

Alkali metals

Alkali earth metals

Front 66

P block elements contain groups ___,___,___,___,___,___

And consist of _____, _____ and ____

Back 66

IIIA , IVA, VA, VIA, VIIA, VIIIA

metals, metalloids and non metals.

Front 67

Group 8 elements

Back 67

Are noble gases

Don’t mix,

Front 68

Group 7 elements

Back 68

Are halogens

Non metals

Front 69

Group 6 elements

Back 69

Non metals, metalloids and metals

Front 70

What is an ion?

Back 70

An atom or molecule with a net electric charge due to the loss or gain of one or more electrons