Ch 8 Notes

Question 1

Electron Spin

Answer 1

4th Quantum Number

Electron spin magnetic quantum number

Question 2

Magnetic behavior of electrons

Answer 2

Electrons behave as though they have a spin

Because of the spin the electron acts as a micro magnet creating a tiny magnetic field

Question 3

Diamagnetic

Answer 3

Slightly repelled by a strong magnet

All of the electrons are paired

Question 4

Paramagnetic

Answer 4

Attracted by a strong magnet

Paramagnetism arises from the spin of electrons

Question 5

Spin can be thought of as quantized

Answer 5

Electrons are paired (and have opposite spins)

Question 6

The spins of two electrons in an orbital do what to each other?

Answer 6

The paired spins cancel each other out

Question 7

PARAMAGNETISM

Answer 7

The attraction of a substance to a magnet
Arises from the spin of electrons
Ions or elements must have at least 1 unpaired electron

Question 8

Pauli Exclusion Principle

Answer 8

No two electrons in an atom can have the same four quantum numbers
Therefore no atomic orbital can contain more than two electrons

Question 9

Orbital Box Diagrams

Answer 9

Represent electron configurations by placing arrows in boxes showing the direction of the spin

Question 10

Aufbrau Principle

Answer 10

Electrons fill the shells from the lowest possible energy and up
Electrons fill shells so that the total energy of the atom is the lowest possible

Question 11

For two subshells with the same value of “n+l” electrons do what?

Answer 11

Electrons are assigned first to the subshell of lower “n”

Question 12

Effective Nuclear Charge

Z

Answer 12

The nuclear charge experienced by a single electron (in a multi-electron atom) which is effected by the presence of other atoms

Question 13

The net positive charge attracting the electron is called the effective nuclear charge

Answer 13

Inner electrons can shield outer electrons from the charge of the nucleus

Question 14

“Z” decreases with increasing “l”

Answer 14

Outer electrons are less tightly held to the atom

Question 15

Degenerate

Answer 15

Orbitals in the same subshells with the same energy

Question 16

Atomic Electron Configurations

Answer 16

spdf notation
orbital box notations
configurations - elements position on table - chemical properties

Question 17

Noble Gas Notation

Answer 17

[He] 2s1

Elements in brackets are considered “core electrons”

Question 18

What are valence electrons?

Answer 18

Electrons beyond the core

Question 19

Hunds Rule

Answer 19

The most stable arrangement of electrons is with the maximum number of unpaired electrons all with the same spin
Fill orbitals with the same direction of spin first

Question 20

What do the letter blocks tell?

Answer 20

They tell the orbital location for the outermost electron for that element

Question 21

Transition elements fill what subshells?

Answer 21

The “d” subshells

Question 22

How are cations formed?

Answer 22

By the removal of one or more valence electrons
Removal order p-(t)-s-d
pre-test-stress-disorder

Question 23

Similar properties of elements are the result of what?

Answer 23

Similar valence electron configurations

Question 24

Atomic Size

Answer 24

Distance between atoms in a sample of the element

Radius is 1/2 the distance between two nuclei

Question 25

Periodic Trends of Atomic Size

Main Group Elements

Answer 25

Atomic radii increases going down a group (n is increasing)
Atomic radii decreases going down a period (core electrons stay the same)
Effective Nuclear Charge increases so atomic radius decreases
Size is determined by outermost electrons

Question 26

Transition Metal Trends of Atomic Size

Answer 26

Filling of “d” orbitals effects the trend
Increase in E.N.C. is almost negated by the repulsion of electrons in the “d” orbitals
Radii decrease, level out, then slightly increase

Question 27

What is Ionization Energy?

Answer 27

The energy required to remove an electron from the atom

POSITIVE because energy is required

Question 28

Periodic Trends of Ionization Energies

Main Group Elements

Answer 28

Increase across - Increasing E.N.C
Decrease down - electron is increasingly farther away from the nucleus
Varies from “s” to “p” block and from half filled orbitals

Question 29

Electron Affinity

Answer 29

the energy of a process in which an electron is acquired by the atom in the gas phase
Greater Affinity - More Negative EA
atoms that attract electrons to from negative ions

Question 30

Electron Affinity and Ionization Energy and E.N.C

Answer 30

Generally a high ionization energy means a high electron affinity
Affinity increases across because of increasing effective nuclear charge
Affinity decreases down because electrons are generally farther away from the nucleus

Question 31

Ion Sizes

Decreases as protons increase
E.N.C is the determining factor in size

Answer 31

Cations are smaller becuase the nucleus is acting on one less electron
Change in size is greatest when electron removed is last in a shell
Anions are larger becuase of increased electron repulsions

Question 32

Isoelectronic Ions

Answer 32

Ions with the same number of electrons but with a different number of protons