Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry 1A > Week Four > Flashcards

Week Four Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

ionisation energy

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

ionisation energy - more than 1 time

A

more energy is required for each time you remove an electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

zeff increase

A

number electron decrease

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Ionisation energy trends

A

increases left to right

decreases down a group

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Electron Affinity

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Metallic CHaracter trends

A

increase down a group

decreases across a period

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

metals form

A

cations

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Non metals form

A

anions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

metal + metal

A

metal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Metal + non metal

A

ionic compound

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Non metal + non metal

A

covalent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Metallic Bonds

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Covalent Bonding

A

reduction in potential and kinetic energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Eb

A

bond energy (between peak and midline)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Covalent bond drawing

A

a horizontal line between 2 atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

unequal sharing of electrons

A

one atom has significantly higher nuclear charge

unsymmetrical distrubution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Electronegativity

A

abilityof atom to attract electrons

greater for non metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Electronegativity trends

A

increases left to right

decreases down

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

ionic

A

more electrons so greater charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Non polar covalent

A

similar electronegativites, shares electron equally

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Polar covalent

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Polarity

A

determined by difference between electronegativity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Lone Pairs

A

not involved in bonding

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Bonding pairs

A

valence electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Lewis Structures

A

valence electron arrangement

only outer shell interact

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

VSEPR

A

prediction of molecule geometry

27
Q

Molecular Orbital Theory

A

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

28
Q

Octet rule

A

wants 8 electrons, gains, loses or shares

29
Q

Formal charge

A

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

30
Q

Electrostatic energy

A

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

31
Q

Coulomb’s law

A

E(electrostatic) - k(Q1Q2/r)

- describes potential energy of 1 pair of electrons

32
Q

k

A

9.00 x 10^9

33
Q

Q1 and Q2

A

charge of separate species

34
Q

R

A

separation distance

35
Q

electron - nuclei interactions

A

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

36
Q

Electron - Electron interaction

A

repel

raises energy and reduces stability

37
Q

Nuclei - Nuceli Interaction

A

repel

interactions reduce stability

38
Q

Bond length trend

A

become longer as atom size increases

39
Q

bond length

A

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

40
Q

bond length - polarity

A

polarity contributtes because partical charges generate electrostatic attracion

41
Q

bond length - multiple bonds

A

shorter than single bond

42
Q

Bond energy

A

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

43
Q

bond energy - trend

A

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

44
Q

sigma bond

A

symmetric bond with respect to rotation around internucleas axis

45
Q

Lattice energy

A

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

46
Q

Formal charge

A

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

47
Q

VSEPR

A

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

48
Q

two sets of electron pairs

A

linear

180*

49
Q

three sets of electron pairs

A

trigonal planar

120*

50
Q

Four sets of electron pairs

A

tetrahedral

109.5*

51
Q

Five sets of electron pairs

A

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*

52
Q

Six sets of electrons

A

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

53
Q

Dipole Moment

A

one end slightly postive one end slightly negative

54
Q

Orbital overlap

A

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

55
Q

Hybrid orbitals

A

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

56
Q

Molecular Orbital Thoery

A

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

57
Q

Inphase overlap

A

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

58
Q

Out of phase overlap

A

desctructive, gives molecular orbital zero amplitude and zero electron density

59
Q

node

A

where amplitude changes

60
Q

bond order

A

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

61
Q

Sp3 hybrid - shape

A

tetrahedral

62
Q

sp2 hybrid - shape

A

Trigonal

63
Q

Sp hybrid - shape

A

linear

Chemistry 1A (12 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions