Notes from slides

Question 1

What happens to the distance between orbits from the nucleus

Answer 1

The distance between orbits decreases with distance from the nucleus

Question 2

What happens to the energy as the distance increases from the nucleus

Answer 2

more energy

Question 3

Name the waves on electromagnetic spectrum

Answer 3

gama, X ray, UV VBGYOR IR micro radio
highest to lowest energy
short to long wavelength

Question 4

Rank the subshells in order of their energy

Answer 4

s < p < d < f

Question 5

Does subshell s have multiple orientations

Answer 5

No, all other except for s do. they can exist in x y z plane

Question 6

How many electrons in each orbital

Answer 6

2, spins up and down

Question 7

What are three rules for electron filling in an atom

Answer 7

Pauli principle - describes the carrying capacity of orbitals. No two electrons can be identical. This limits the occupancy to max of 2 electrons
Aufbau principle - electrons are added to orbitals from lowest to highest energy . electrons are removed from valence orbitals first with highest to lowest energy
Hund’s rule - electrons fill degenerate orbitals one per orbital before pairing. paramagnetic and dimagnetic.

Question 8

According to Aufbau principle, what are the rules to fill electrons in subshells 4s and 3d

Answer 8

Even though 3d is higher in energy than 4s, the valence electrons are removed from 4s first before 3d.

Question 9

What are the rules for excited state electron configurations

Answer 9

make sure the configuration has the correct total number of electrons

the electrons can be in any orbital as long as that orbital exists.

Question 10

Difference between the Aufbau principle and Hund’s rule

Answer 10

Aufbau principle describes how electrons are added/removed from orbitals of different energy however Hund’s rule describes how electrons are added/removed from the orbitals of the same energy

Question 11

Half filled/fully filled orbitals are higher in energy?

Answer 11

false, lower in energy

Question 12

Define paramagnetic

Answer 12

at least one unpaired electron

Question 13

Define diamagnetic

Answer 13

all the electrons are paired

Question 14

What are the 7 element groups

Answer 14

group 1 - alkali metals
group 2 - alkaline earth metals
group 7 - halogen
group 8 - noble gases
the d block - transitional metal
the s and p blocks - representative elements
the f block - rare earth metals

Question 15

Describe the shielding effect

Answer 15

core electrons shield the valence electrons from the full nuclear charge
more core electrons, less attracted the valence electron is to nucleus

Question 16

What is effective nuclear charge

Answer 16

the nuclear charge experienced by a valence electron

Question 17

moving down a group, what happens to electrostatic force (F e), size and nuclear charge (Z eff)

Answer 17

F e decreases, Z eff is constant because core electrons are added at the same rate as protons, r increases

Question 18

moving across a period, what happens to electrostatic force (F e), size and nuclear charge (Z eff)

Answer 18

F e increases, size remains constant, Z eff increases because core electrons remain constant while protons are added.

Question 19

moving from positive to negative charge, what happens to electrostatic force (F e), size, charge (C) and nuclear charge (Z eff)

Answer 19

F e decreases with increasing negative charge, C becomes negative, size doesnt change much, Z eff remains constant because core electrons and protons remain the same

Question 20

Atomic radius moving from left to right

Answer 20

decreases (Fe increases)

Question 21

Atomic radius form top to bottom

Answer 21

increases

Question 22

How does ionic radius change with charge

Answer 22

ionic radius increases with negative charge

Question 23

Ionization energy

Answer 23

minimum amount of energy required to remove the outer most electron from an atom in its gaseous state. depends on F e

Question 24

left to right, ionization energy

Answer 24

F e increases so IE increases

Question 25

Top to bottom, ionization energy

Answer 25

Fe decreases, IE decreases

Question 26

What are the rules for multiple ionizations

Answer 26

1. more positive charge on an ion (cation), more ionization energy
2. second IE is greater than first IE
3. pulling off electron from a half full/full orbital require more IE

Question 27

Define electron affinity

Answer 27

energy change when adding an electron to valence shell of an atom in its gaseous state. exothermic. More Fe, more energy is released

Question 28

Electron affinity left to right

Answer 28

F e increases left to right, more negative because more energy is released

Question 29

Electron affinity top to bottom

Answer 29

Fe decreases top to bottom, therefore less negative EA because less energy is released.

Question 30

Electronegativity and Fe

Answer 30

As Fe increases ENV increases, from left to right and bottom to top

Question 31

Pneumonic for ENV

Answer 31

FONClBrISCH

Question 32

acidity from left to right

Answer 32

as stability increases of the anion (conjugate base) produced increases, the acidity increases. as the size of the anion increases, the stability increases. Left to right, size increases and acidity also increases

Question 33

Acidity top to bottom

Answer 33

top to bottom the size increases and so does the acidity