Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Structure > Flashcards

Structure Flashcards

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

Name compounds, elements or ions which are tetrahedral.

A

Methane 109.5
Ammonium ion 109.5
Sulfate ion 109.5

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

Name compounds, elements or ions which are trigonal planar

A

Boron trichloride 120
Carbonate ion 120
Nitrate ion 120

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

Name compounds, elements or ions which are bent

A

Water 104.5

Sulfur dioxide 120

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

Name compounds, elements or ions which are trigonal bypyrimidal

A

Phosphorus pentachloride (in gas phase) 90 & 120

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

Name compounds, elements or ions which are pyramidal

A

Ammonia 107

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

Name compounds, elements or ions which are octahedral

A

Sulfur hexafluoride 90

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

Name compounds, elements or ions which are linear + state their bond angle

A

Carbon dioxide 180
Beryllium chloride 180
Hydrogen Chloride 180

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

Why is sulfur dioxide bent?

A

The lone pair and a bonding pair repel more than a bonding pair and a bonding pair

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

Why is ammonia pyramidal?

A

There are 3 bonded pairs and one lone pair of electrons. The bonded pairs repel less with each other than the lone pair and the bonded pair which results in a pyramidal shape.

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

Marking points for why one angle MAY be smaller than the other?

A

Extra lone pair
Lone pairs repel more
Bonding pairs are pushed closer together

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

Why are bond angles the angle they are?

A

to minimise repulsion of electron pairs

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

equation for working out the number of lone pairs

A

1/2 x [group number of the element - number of covalent bonds (not including covalently bonded lone pairs bc don’t know what they are!]

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

go to phrase about repulsions

A

lone pair-lone pair repulsions are greater than lone pair-bonding pair repulsions which are greater than bonding-bonding pair repulsions

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

analogous molecules to:

1) CH4
2) NH3
3) H2O

A

1) CH4 —> SiH4
2) NH3 —> PH3
3) H2O —-> H2S

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

How many lone pairs does ammonia (NH3) have?

A

1

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

How many lone pairs does wat have?

A

2

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

How many lone pairs does sulphur dioxide (SO2) have?

A

1

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

carbonate and nitrate ions both have…

A

two single bonds, one double (two snakes, one den)

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

SO4 2- drawing has…

A

a wedge
a dash
two double bonds

20
Q

What to always say about electron repelling? ?????

A

electrons repel to MINIMISE REPULSION ??????? check tutorial answers

21
Q

how many degrees does one pair of lone electrons decrease bond angle by?

A

2.5 degrees

22
Q

complex shapes

A

variations of octahedral and trigonal bypyramidal where some bonds are replaced with lone pairs

23
Q

4 divisions of structures for solids

A

1) giant ionic
2) giant covalent
2) metallic
3) simple molecular

24
Q

Giant ionic lattices (two examples and diagram description)

A

sodium chloride, magnesium oxide

cubic structure with alternating atoms (see chemrevise + practice drawing)

25
Q

Giant covalent (two examples + description)

A

diamond (C) - tetrahedral arrangement of C atoms - each C covalently bonded to 4 other C’s
tower -ish drawing

Graphite (C) - planar arrangement of C atoms in layers (hexagons)
C covalently bonded to three other C’s
4th outer electron in each C atom is delocalised. Delocalised electrons present between layers

silicon (IV) oxide / silicon dioxide (same thing) - SiO2

(see chemrevise + practice drawing)

26
Q

Bonds in giant covalent structures

A

strong covalent bonds = high melting points

27
Q

Metallic structure drawing

A

2D lattice drawing (showing closely packed ions and delocalised e-)

28
Q

Simple molecular diagram

A

Eg. regular arrangement of I2 molecules held together by weak london forces
diagram: lots of I-I’s floating about

Ice
draw H2O as though sticking left arm up and right arm out to the right then draw Hydrogen bonds between the oxygen’s two lone pairs and hydrogens branching out to the left (these hydrogens are attached to the rest of two different water molecules)
-tetrahedral arrangement
-molecules held further apart

(see chemrevise)

29
Q

Properties of diamond

A
  • cannot conduct electricity because all four electrons per atom are involved in covalent bonds
  • localised electrons, cannot move
30
Q

Properties of graphite

A
  • giant covalent
  • can conduct electricity because one electron per carbon is delocalised and free to move along layers
    BUT doesn’t conduct electricity BETWEEN layers because the energy gap between them is too large for an easy electron transfer
31
Q

Graphene

A
  • a single one-atom-thick layer of graphite (3 covalent bonds per C atom and a 4th electron per atom which is delocalised).
  • thin, nearly transparent sheet
  • high tensile strength due to strong covalent bonds
  • can conduct electricity because one electron is free and delocalised
32
Q

C60 - Buckminster Fullerene

A
  • hexagons and pentagons

- red + soluble in organic liquids

33
Q

Carbon Nanotubes

A
  • used in drug delivery
  • tubular structures made from carbon hexagons
  • can conduct electricity along tube because one electron per carbon is delocalised and free
34
Q

solid to gas

A

sublimation

35
Q

Why is graphite used as a solid lubricant?

A

layer slide over each other easily

due to weak forces between the layers

36
Q

NO3 - is an example of a what covalent bond

A

dative covalent

One double bond
two single bonds, one drawn showing an arrow to represent dative

37
Q

tetrahedral bond angle

A

109.5

plosive tet and NINE.5

38
Q

trigonal planar bond angle

A

120

360/3 = planar = 120

39
Q

bond angle definition

A

geometric angle between two adjacent bonds

40
Q

what is the degree of the C-C-C bond angle in diamond?

A

109.5

41
Q

Diamond one word shape

A

TETRAHEDRAL

42
Q

Graphite one word shape

A

HEXAGONAL

43
Q

Buckminster fullerene two word shape

A

HEXAGONS AND PENTAGONS

44
Q

Ice one word shape

A

TETRAHEDRAL (internet say hexagonal as well)

45
Q

carbon nanotubes one word shape

A

HEXAGONS

46
Q

Go to phrase about bonding pairs only

A

BONDING PAIRS ARE PUSHED CLOSER TOGETHER

47
Q

How many lone pairs does the wired anomaly shape SF4 have?

A

one

Chemistry (37 decks)

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