Week Four

Question 1

ionisation energy

Answer 1

strength with an atom holds its electon in a indicator of chemical property

Question 2

ionisation energy - more than 1 time

Answer 2

more energy is required for each time you remove an electron

Question 3

zeff increase

Answer 3

number electron decrease

Question 4

Ionisation energy trends

Answer 4

increases left to right

decreases down a group

Question 5

Electron Affinity

Answer 5

energy change when atom accepts a proton to from ion
becomes more exothermic moving to right hand side
little change down group

Question 6

Metallic CHaracter trends

Answer 6

increase down a group

decreases across a period

Question 7

metals form

Answer 7

cations

Question 8

Non metals form

Answer 8

anions

Question 9

metal + metal

Answer 9

metal

Question 10

Metal + non metal

Answer 10

ionic compound

Question 11

Non metal + non metal

Answer 11

covalent

Question 12

Metallic Bonds

Answer 12

in solid metals
bonded to several atoms
electrons are free to move which is why they have high electical conduction

Question 13

Covalent Bonding

Answer 13

reduction in potential and kinetic energy

Question 14

Eb

Answer 14

bond energy (between peak and midline)

Question 15

Covalent bond drawing

Answer 15

a horizontal line between 2 atoms

Question 16

unequal sharing of electrons

Answer 16

one atom has significantly higher nuclear charge

unsymmetrical distrubution

Question 17

Electronegativity

Answer 17

abilityof atom to attract electrons

greater for non metals

Question 18

Electronegativity trends

Answer 18

increases left to right

decreases down

Question 19

ionic

Answer 19

more electrons so greater charge

Question 20

Non polar covalent

Answer 20

similar electronegativites, shares electron equally

Question 21

Polar covalent

Answer 21

One is more electronegative than the other so one has partially negative charged while other is partially positive

Question 22

Polarity

Answer 22

determined by difference between electronegativity

Question 23

Lone Pairs

Answer 23

not involved in bonding

Question 24

Bonding pairs

Answer 24

valence electrons

Question 25

Lewis Structures

Answer 25

valence electron arrangement | only outer shell interact

Question 26

VSEPR

Answer 26

prediction of molecule geometry

Question 27

Molecular Orbital Theory

Answer 27

describes the type of atomic orbitals used to share ore hold lone pairs

Question 28

Octet rule

Answer 28

wants 8 electrons, gains, loses or shares

Question 29

Formal charge

Answer 29

(number of valence electrons in free atom) - (number of non bonding valence electrons) - 1/2 (number of bonding electrons)

Question 30

Electrostatic energy

Answer 30

2 charged species is proportional to magnitudes of charges and innversely proportional to distance between them

Question 31

Coulomb's law

Answer 31

E(electrostatic) - k(Q1Q2/r) | - describes potential energy of 1 pair of electrons

Question 32

k

Answer 32

9.00 x 10^9

Question 33

Q1 and Q2

Answer 33

charge of separate species

Question 34

R

Answer 34

separation distance

Question 35

electron - nuclei interactions

Answer 35

electrons and nuclei attract one another attractions are energetically favourable at lower energy than free electron

Question 36

Electron - Electron interaction

Answer 36

repel | raises energy and reduces stability

Question 37

Nuclei - Nuceli Interaction

Answer 37

repel | interactions reduce stability

Question 38

Bond length trend

Answer 38

become longer as atom size increases

Question 39

bond length

Answer 39

the separation distance at which a molecule has the maximum energetic advantage over the atoms

Question 40

bond length - polarity

Answer 40

polarity contributtes because partical charges generate electrostatic attracion

Question 41

bond length - multiple bonds

Answer 41

shorter than single bond

Question 42

Bond energy

Answer 42

energy required to break bonds, multiply energy of single bonds by avogadros

Question 43

bond energy - trend

Answer 43

increases as more electrons are shared increases as electronegativity difference increases decreases as bond gets longer

Question 44

sigma bond

Answer 44

symmetric bond with respect to rotation around internucleas axis

Question 45

Lattice energy

Answer 45

energy change on converting 1 mole of ionic solid into ions, depending on charges

Question 46

Formal charge

Answer 46

charge atom would have if each its bonding electrons werre equally shared

Question 47

VSEPR

Answer 47

minimising electron electron repulsion by placing electron pairs as far apart as possible,

Question 48

two sets of electron pairs

Answer 48

linear | 180*

Question 49

three sets of electron pairs

Answer 49

trigonal planar | 120*

Question 50

Four sets of electron pairs

Answer 50

tetrahedral | 109.5*

Question 51

Five sets of electron pairs

Answer 51

trigonal bipyrimid | 3 are positioned in corners of triangle 120* from one another and the 2 others are above and below centre atom at 90*

Question 52

Six sets of electrons

Answer 52

octahedral sit at 6 vertices of octahedron 90* and 180*

Question 53

Dipole Moment

Answer 53

one end slightly postive one end slightly negative

Question 54

Orbital overlap

Answer 54

when 2 orbitals of same phase are superimposed, results in new orbital

Question 55

Hybrid orbitals

Answer 55

atomic orbitals obtained by combining 2 or more valence orbitals - has to be 2 different energy levels

Question 56

Molecular Orbital Thoery

Answer 56

overlap of 2 atomic orbitals leads to the formation of one bonding orbital and one antibonding orbital.

Question 57

Inphase overlap

Answer 57

constructive and results in formation of molecular orbital with large amplitude and high electron density

Question 58

Out of phase overlap

Answer 58

desctructive, gives molecular orbital zero amplitude and zero electron density

Question 59

node

Answer 59

where amplitude changes

Question 60

bond order

Answer 60

1/2 (number of electrons in bonding molecular orbitals - number of electrons in antibonding molecular orbitals)

Question 61

Sp3 hybrid - shape

Answer 61

tetrahedral

Question 62

sp2 hybrid - shape

Answer 62

Trigonal

Question 63

Sp hybrid - shape

Answer 63

linear