Bonding 1

Question 1

Oxidation states

Answer 1

Helps keep track of the electro distribution between variius reactants and products in a chemical reaction

Question 2

Element is oxidized when

Answer 2

The oxidation number of the element becomes more positive during s chemical reaction

Question 3

Element becomes reduced when

Answer 3

The oxidation number becomes more negative during s chemical reaction

Question 4

Ground state

Answer 4

When all electrons are in the lowest energy orbitals available

Question 5

Closed shell

Answer 5

A condition referred to as an octet when considering s and p valence electrons

Question 6

Valence Shell Electron Pair Repulsion (VSEPR) Theory

Answer 6

Predicts shape of simple molecules; one rule = electron pairs, whether bonding or non bonding, attempt to move as far apart as possible

Question 7

Linear

Answer 7

A molecule with a 180 bond angle

Question 8

Electron groups

Answer 8

Determine the atom’s geometric identity

Question 9

2 electron groups

Answer 9

Linear

sp hybridization

Question 10

3 electron groups

Answer 10

Trigonal planar

sp2 hybridization

Question 11

4 electron groups

Answer 11

Tetrahedral

sp3 hybridization

Question 12

5 electron groups

Answer 12

Triagonal bipyramidal

dsp3 hybridization

Question 13

6 electron groups

Answer 13

Octahedral

d2sp3 hybridization

Question 14

Determining molecular shape

Answer 14

1. ) count number of electron groups = geometric family

2. ) determine shape based on non binding pairs

Question 15

Determining hybridization

Answer 15

Orbitals always get used up s -> d; start left and work right until all orbitals are filled;
Hybridization of carbon on Methane = s+p+p+p = sp3

Question 16

Covalent bond

Answer 16

Atoms attempt at closed shell stability; it is two atoms with similar electronegativities compromise to achieve octet

Question 17

Nonpolar bonds

Answer 17

Covalent bonds in which the electron pair spends the same amount of time around each atom

Question 18

Polar bonds

Answer 18

Covalent bonds that are fatter at one end than at the other

Question 19

Band theory

Answer 19

Model in which the metal is thought of as a giant molecule in which delocalized molecular orbitals cover the entire structure

Question 20

Continuous band

Answer 20

Formed when N molecular orbitals are very closely spaced in energy and form a band covering a range of energies

Question 21

Valence band

Answer 21

Band that is the highest energy and contains freely moving valence electrons

Question 22

Conduction band

Answer 22

The empty band that overlaps the valence band; if electrons jump into it the material will be able to conduct electricity

Question 23

Band Theory point 1

Answer 23

When a valence band is not fully occupied, valence electrons can move in many energy states

Question 24

Band theory point 2

Answer 24

Valence electrons can jump into the conduction band

Question 25

Band theory point 3

Answer 25

The width of the band depends of the degree of overlap of the atomic orbitals between neighboring atoms: the greater the overlap the wider the band

Question 26

Band theory point 4

Answer 26

A band is thus a near-continuum of finite number of energy levels

Question 27

Band theory point 5

Answer 27

The band constructed from the overlap of s orbitals is called the s band. Similarly p bands and d bands can be constructed

Question 28

Band theory point 6

Answer 28

A metal has overlapping valence and conduction band (VB and CB)

Question 29

Band theory point 7

Answer 29

Insulators have a big gap between their VB and CB

Question 30

Band theory point 8

Answer 30

A semiconductor has a small gap between the VB and CB; adding energy can then excite electrons that can jump from VB to CB