Atomic Theories

Question 1

How did bohr expnd on rutherfords theory of the atom?

Answer 1

Quantized the shells

Question 2

Electron ins ground state vs excited state

Answer 2

Ground has lower enegery

Question 3

When an electron falls from higher engery level to lower enegry levels, how is energy released?

Answer 3

as a photon

Question 4

Difference between previous model of atom vs modern quantum mechanical model?

Answer 4

2D vs 3D

Question 5

Further from the nucleus the ____ energy an electron has.

Answer 5

More

Question 6

region of space in which high probablity of finding an electron

Answer 6

Orbital

Question 7

term used to label energy levels of electrons

Answer 7

n=

Question 8

How are s orbitals different from p orbitals

Answer 8

different shape s =O p= 8

Question 9

How does atom valence elctron configuration determine place on periodic table?

Answer 9

Valence determines block or group number

Question 10

What two elements are exceptions to the way we normally write electron configurations? Write
the expected and the actual confi uration of each. What rules are followed? What ru es are
violated?

Answer 10

Cu= [Ar] 4s1 3d10
Cr= [Ar]4s0 3d5
full subshells are stable

Question 11

Transition metals

Answer 11

titanium, chronium, mecury

Question 12

Discovered the nucleaus

Answer 12

Ruther

Question 13

Cathode ray tubes

Answer 13

Ruther

Question 14

Discovered proton

Answer 14

Ruther

Question 15

Most of atom empty space

Answer 15

Rutherford

Question 16

Partial Positive

Answer 16

if something is a partial positive it’s electronegativity will be less than the other elements electronegativity
•if the molecule has more than two elements you look at the individual bonds

Question 17

Partial Negative

Answer 17

if something is a partial negative it’s electronegativity will be higher than the other elements

Question 18

Polar Bonds

Answer 18

to know if a molecule has polar or non-polar bonds you look at the difference in electronegativity
•if the difference is above 0.3 its polar bonds
•if the difference is below 0.3 its non-polar bonds

Question 19

Polar Molecules

Answer 19

to know if a molecule is polar or non-polar, you can look at its symmetry
•if its symmetrical the molecule is non-polar
•if its asymmetrical the molecule is polar

Question 20

London Forces

Answer 20

if the molecule is non-polar you will only have london forces

Question 21

Dipole Dipole

Answer 21

if the molecule is polar you will have dipole dipole forces (only if you don’t have hydrogen bonds)

Question 22

Hydrogen Bonds

Answer 22

if you only have a H with a 𝒮+and a N, O, or F with a 𝒮- you will have a hydrogen bond

Question 23

Density Formula

Answer 23

Mass/ Volume

Question 24

Ion

Answer 24

an atom that loses or gains electrons (to form a full valence shell) and results in a charge. It is a charged particle.

Question 25

Cations

Answer 25

lose electrons
become more positive

Question 26

Anions

Answer 26

gains electrons
becomes more negative

Question 27

Orbitals

Answer 27

3D space around a nucleus where there is a probability of finding electrons.

Question 28

S subshell

Answer 28

Principal Energy Level: +1
Shape: spherical
# of orbitals: 1
Max # of Electrons: 2

Question 29

P subshell

Answer 29

Principal Energy Level: +2
Shape: Dumbell like
# of orbitals: 3
Max # of Electrons: 6

Question 30

D subshells

Answer 30

Principal Energy Level: +3
Shape: vary
# of orbitals: 5
Max # of Electrons: 10

Question 31

F subshells

Answer 31

Principal Energy Level: +4
Shape: Vary
# of orbitals: 7
Max # of Electrons: 14

Question 32

Aufbau Principal

Answer 32

each electron is added to the lowest energy level available.

Question 33

Hund’s Rule

Answer 33

for orbitals at the same energy level, one electron occupies each sub orbital before the electrons pair up.

Question 34

Pauli Exclusion Principal

Answer 34

only two electrons (with opposite spins) can occupy each orbital

Question 35

Lewis Bonding Theory

Answer 35

atoms/ions are stable if they have an octet of electrons •electrons are most stable in pairs
•atoms form chemical bonds (ionic or covalent) to become stable

Question 36

VSEPR Theory

Answer 36

VSEPR (Valence Shell Electron Pair Repulsion)
•valence electrons stay as far away as possible to minimize repulsion
•when looking at a molecule we look specifically at the central atom (the one that has the most bonding electrons) to determine the 3-D geometry