Brainscape's Knowledge GenomeTM

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


See full index

chem > module 2.2 up to 2.2.8 > Flashcards

module 2.2 up to 2.2.8 Flashcards

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

Does energy of shells increase or decrease as you move away from the nucleus?

A

increase

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

what is the principal quantum number?

A

n

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

what is the formula for the maximum number of electrons a shell can hold?

A

2n^2

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

where are electrons found?

A

in atomic orbitals

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

what is an atomic orbital?

A

a region around the nucleus which can hold up to 2 electrons with opposite spins (upspin & downspin)

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

what are the 4 orbitals?

A

s p d f

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

how many s orbitals are there per shell?

A

1

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

how many p orbitals are there per shell?

A

3, found in 2 and above

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

how many d orbitals are there per shell?

A

5, found in 3 and above

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

how many f orbitals are there per shell?

A

7, found in 4 and above

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

what are the max number of electrons per shell?

A

2,8,18,32…

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

what is the shape of an s orbital?

A

spherical

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

what is the shape of an p orbital?

A

dumb-bell

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

what is a subshell?

A

all of the orbitals of the same type in the same shell

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

what fills before 3d (electron configuration)

A

4s

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

why don’t orbitals pair when going into boxes immediately?

A

they only pair when they have to

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

what is the electron configuration for cobalt (27)?

A

1s2 2s2 2p6 3s2 3p6 4s2 3d7

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

~why are orbitals not filled in numerical order?

A

because the principal energy levels get closer together as you go further from the nucleus

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

what does an ion have the same of but a different amount of

A

ion-same amount of protons, different amount of electrons

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

what type of ion does oxygen form?

A

oxide ion

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

what type of ions do metals form?

A

positive ions (cations)

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

what type of ions do non-metals form?

A

negative ions (anions)

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

what is the electron configuration of sodium(11) and the sodium ion?

A

sodium: 1s2 2s2 2p6 3s1

na+:1s2 2s2 2p6

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

what do you notice about the electron configuration of ions?

A

all ions have the same electron configuration as noble gasses.

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

write the shorthand configuration of Na

A

[Ne]3s1

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

as the 4s shell fills first…

A

it is always first to empty ( eg for ions)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

what is an ion

A

an atom that has gained or lost electrons- it possess a positive or negative charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

what group changes their name when becoming ions

A

halogens

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

what is the name of fluorine when it becomes an ion

A

fluoride

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

what is the name of nitrogen when it becomes an ion

A

nitride

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

what is the name of chlorine when it becomes an ion

A

chloride

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

what is the formula of the complex ion: nitrate

A

NO3-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

what is the formula of the complex ion: sulfate

A

SO4^2-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

what is the formula of the complex ion: hydroxide

A

OH-

35
Q

what is the formula of the complex ion: carbonate

A

CO3^2-

36
Q

what is the formula of the complex ion: Ammonium

A

NH4+

37
Q

what is the formula of ammonia

A

NH3

38
Q

what is the formula of the sulfide ion

A

S^2-

39
Q

how many ions can transition metals form?

A

more than 1

40
Q

how are ionic compounds formed?

A

when ions of opposite charge come together to form ionic compounds.

41
Q

what are spectator ions?

A

ions that are present during a reaction but remain unchanged (present on both sides of the reaction).

42
Q

Describe the structure of ionic compounds and how it occurs…

A
  • oppositely charged ions attract each other (from all directions).
  • each of these ions in turn attract more ions to form a giant lattice structure (lattice=repeating)
  • billions of ions latticed together.
43
Q

talk about the melting/ boiling points of ionic substances and why this is.

A

high melting/boiling points as it requires a large amount of ENERGY to break the many STRONG ELECTROSTATIC BONDS between IONS in the GIANT LATTICE STRUCTURE.

44
Q

do ionic compounds conduct electricity when melted?why?

A

yes, high temp= enough energy to overcome the many strong forces of attraction between ions. Ions are free to move around within the molten compound so conducts electricity.

45
Q

do ionic compounds conduct electricity when solid?why?

A

no, ions are fixed in position in giant lattice, can vibrate but not move so cant conduct

46
Q

do ionic compounds conduct electricity in solution?why?

A

yes, water molecules separate ions from the lattice. Ions are free to move around in the solution, it does conduct electricity.

47
Q

what do many ionic compounds dissolve in?

A

polar solvents eg water

48
Q

why do ionic compounds dissolve in polar water molecules.

A

polar water molecules break down the lattice and surround each ion in solution

49
Q

why might water not be able to break up a compound of ions with large charges?

A

the ionic attraction may be too strong so lattice structure not broken down- compound=not very soluble

50
Q

when do ionic compounds have a lower solubility?

A

when ions hold onto each other more firmly( stronger attraction because larger charge)

51
Q

what are isotopes

A

atoms of the same atomic number (protons) but a different mass number (neutrons)

52
Q

~what is Ar/Mr

A

relative atomic mass/ relative molecular mass

53
Q

how do u calculate Ar (isotopes)

A

Ar= (isotope mass x percentage)+(isotope mass x percentage)/100

54
Q

are covalent bonds strong?

A

yes

55
Q

why are covalent bonds strong?

A

because of the ELECTROSTATIC forces between the shared negatively charged electrons and the positively charged protons in the nucleus of each atom

56
Q

state how covalent bonds are formed…

A

covalent bonds are formed when orbitals, each containing one electron overlap. this forms a region in space where an electron pair can be found

57
Q

the greater the overlap of oribitals, the stronger the…

A

… bond

58
Q

talk about the covalent attraction of H2

A

in H2, the attraction is soley between the shared pair of electrons in the covalent bond and the nuclei of the atoms~

59
Q

how many covalent bonds does nitrogen form?

A

3

60
Q

whats it called when nitrogen contributes both electrons in the double bond?

A

coordinate bond/ dative covalent bonds

61
Q

whats a dative covalent bond?

A

a shared pair of electrons where BOTH electrons have been donated by one atom

62
Q

what does average bond enthalpy serve as

A

a measurement of covalent bond strength.

63
Q

describe the melting/boiling points of simple covalent structures

A
  • have weak intermolecular forces so not a lot of energy to break
  • covalent bonds within the molecules are strong and cant be broken easily.
64
Q

are simple covalent structures good at conducting electricity? why?

A

NO because there are no mobile charge carriers, ions or electrons to carry electric charge

65
Q

what are simple covalent structures soluble in?

A

non-polar substances such as hexane

66
Q

name 4 giant covalent structures…

A

diamond, silicon dioxide, graphite, graphene

67
Q

diamond: talk about its melting point

A

high due to network of very strong carbon-carbon covalent bonds which has to be broken before melting occurs

68
Q

diamond: talk about its density

A

v dense due to carbon atoms packed close together

69
Q

diamond: talk about its solubility

A

insoluble in water and organic solvents- no possible attractions

70
Q

why are diamonds rare

A

major heat and pressure needed

71
Q

talk about the formation of graphite

A

each carbon atom forms covalent bonds to 3 other carbon atoms, forming a layer structure

72
Q

graphite: talk about melting point

A

high( lots of energy to break strong covalent bonds)

73
Q

graphite: talk about how it feels

A

soft and slippery as layers of covalently bonded carbon atoms can slide over each other

74
Q

graphite: talk about its solubility

A

insoluble

75
Q

graphite: talk about its conduction of electricity

A

delocalised electrons free to move throughout the sheets carrying charge

76
Q

describe graphene

A

single layer of graphite, strong covalent bonds, excellent electrical conductivity.

77
Q

talk about the solubility of nitrates

A

nitrates are always soluble

78
Q

talk about the solubility of halides

A

halides are soluble with everything except lead, silver and mercury

79
Q

electron config of cr atom

A

1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^5

80
Q

electron config of cr3+ atom

A

1s^2 2s^2 2p^6 3s^2 3p^6 3d^3

81
Q

electron config of copper atom

A

1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^10

82
Q

electron config of cu+

A

1s^2 2s^2 2p^6 3s^2 3p^63d^10

83
Q

electron config of cu2+

A

1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^9

chem (14 decks)

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