Atomic Theory

Question 1

Atomic Theory

Answer 1

All matter is made of atoms- Atoms are indivisible and indestructible

AToms of a specific element are identical in mass and properties

Compounds are formed by whole number ratios

Chemical reactions are rearrangements of atoms

Question 2

Orbitals

Answer 2

Regions of space around nucleus where electrons reisde

Question 3

Heusenberg’s Uncertainty Principle

Answer 3

Impossible to determine both the momentum or location of an electron

Can determine one or the other

Question 4

n

Answer 4

Principle quantum number

Overall energy of orital

Question 5

Max number of electrons that a shell can hold

Answer 5

2n^2

Question 6

l

Answer 6

Azimuthal quantum number
l= 0 to (n-1)

Orbital shape 
0=s
1=p
2=d
3=f

Question 7

m(l)

Answer 7

Magnetic quantum number

Orientation of orbitals in space

= -l to +l

Question 8

m(s)

Answer 8

Spin number

+/- 1/2

Question 9

Pauli Exclusion Principle

Answer 9

No 2 electrons in an atom can have the same set of quantum numbers

Question 10

Aufbau Principle

Answer 10

Lower subshells filled before higher subshell

Question 11

Characteristics of Covalent Bonds

Answer 11

Bond length

Bond energy

Polarity

Question 12

Characteristics of Covalent Bonds- Bond Length

Answer 12

decreases as number of shared electrons increases

Question 13

Characteristics of Covalent Bonds- Bond energy

Answer 13

Energy required to break the bond

Increases as number of shared electrons increases

Question 14

Characteristics of Covalent Bonds-Polarity

Answer 14

Formation of partially charged regions

Question 15

Ionic Bonds

Answer 15

Comlete transfer of electrons across atoms

Held together by electrostatic forces

Question 16

London Dispersion forces

Answer 16

Weakest

Electron density between atoms changes briefly, forming a temporary dipole

Can induce dipoes in neighbouring molecules

In NP compounds

Question 17

Dipole-Dipole

Answer 17

Polar solids and liquids (not gases)

Rearrangement of atoms so that partially positive regions are close to partially negative regions

Question 18

H bonds

Answer 18

Fairly strong

H attracted to O,N.F

Question 19

Bonding Orbitals

Answer 19

Signs of atomic orbitals are the same

Electrons spend most of time between nuclei of 2 atoms (more stable)

Question 20

Anti-bonding orbitals

Answer 20

Signs of atomic orbitals are different

Electrons spend most of time outside of nuclei of 2 atoms (not as stable)

Question 21

Sigma bond

Answer 21

Head to head overlap of orbitals

Question 22

Pi bond

Answer 22

Parallel overlap of orbitals

Can’t rotate

Question 23

Factors Affecting Bond Strength

Answer 23

Bond order

Atomic Radii

Polarity

Lone Pairs

Question 24

Factors Affecting Bond Strength- Bond Order

Answer 24

of bonds

single bond= 1…etc

Higher bond order= lower bond length….. INCREASES bond strength

Question 25

Factors Affecting Bond Strength- Atomic Radii

Answer 25

Increase radius= increased bond length….DECREASES BOND STRENGTH

Question 26

Factors Affecting Bond Strength- Polarity

Answer 26

Increase polarity= INCREASED bond strength

Question 27

Factors Affecting Bond Strength- Lone Paris

Answer 27

Increased LP= DECREASED bond strength

Repulsion between LP weakens bond

Question 28

Hund’s Rule

Answer 28

Electrons must fill up orbitals of the same or different energy levels before pairing up