Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > chemistry topic test 2 > Flashcards

chemistry topic test 2 Flashcards

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

list the properties of metal

A

good conductors of heat and electricity in solid & liquid state

shiny surface

hard

malleable

ductile

insoluble in water

reasonably high MP

very high BP

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

describe metallic bonding

A

particles arranged as a lattice of positive cations surrounded by a sea of delocalised electrons

delocalised: can move around atoms and through the lattice

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

explain the metallic property of heat/electricity conduction

A

when heated energy of cations and delocalised electrons increases

this energy is conducted along metals as cations and electrons collide, transferring electricity

when metals conduct electricity, electrons from one end of the metal cause a similar number of e- to be displaced from the other end

in sold: only electrons move
liquid: both cation and e- carry charge

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

explain the metallic property of malleability and ductility

A

bonding in metals is NON DIRECTIONAL

layers of atoms can slide over each other without destroying metallic bond

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

explain the metallic property of MP & BP

A

MP and BP indicate strength of intermolecular forces

relatively high MP and BP due to strong attraction between positive cations and mobile electrons

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

explain the metallic property of hardness

A

strength of bond is related to charge of positive cations in lattice

metals in group 2 are stronger because atoms release 2 valence electrons (instead of 1 in group 1) and form ions with a +2 charge

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

list the ionic properties

A

non conductors of electricity in solid state

good electrical conductors in molten or liquid state

hard

brittle

relatively high MP

relatively high BP

varying solubilities in water, insoluble in non-polar solvents

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

describe ionic bonding

A

ionic solid:
positive and negative ion are arranged in an orderly 3D lattice

each positive ion is surrounded by negative ions and vice versa

ions are held in fixed positions by strong ionic bonds

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

Explain the ionic property of conducting heat/electricity

A

solid: non conductors because ions are held in a fixed lattice, no mobile charged particles
molten: ions are now mobile, both positive and negative ions carry charge
aqueous: ions dissociate and are able to carry charge

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

Explain the ionic property of MP and BP

A

high MP and BP:

ionic bonding has large electrostatic forces of attraction between holding atoms together in a lattice

large amount of energy is required to overcome strong ionic bonds

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

Explain the ionic property of hardness

A

strong ionic bonding extends throughout lattice solid

scratching requires overcoming strong ionic bonds

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

Explain the ionic property of brittleness

A

ionic lattice doesn’t withstand distortion

when lattice is distorted, like charges align and repel, shattering lattice

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

Describe covalent molecular substances

A

exist only as discrete molecules

non metals only

solid, liquid or gaseous state

intramolecular forces: strong covalent bond hold atoms together within a molecule

intermolecular forces: weak forces of attraction between molecules

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

list the properties of CMS

A

non conductors of electricity in solid and liquid

some are weak/good conductors in aqueous solutions

malleable

soft

low Mp and BP

mostly insoluble in water, soluble in non-polar compounds

examples: F2, H2O, O2

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

explain the covalent molecular property of electricity conduction

A

non conductors in aq, s or l:

molecules are uncharged

electrons are held tightly within covalent bonds

**exception: some CMS react with water to form ions, and become conductors in aqueous solutions

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

explain the covalent molecular property of softness

A

weak intermolecular forces require little effort to overcome: easy to separate molecules

strong covalent bonds aren’t disrupted

17
Q

explain the covalent molecular property of malleability

A

molecules can easily slide or be pushed

only weak intermolecular forced exist between them, these can easily be reformed

18
Q

explain the covalent molecular property of BP and MP

A

low BP and MP:

when CMS are heated, little energy is needed to overcome weak intermolecular forces

19
Q

Describe covalent network substances

A

solid state only

non metals only

carbon with different structures are called allotropes:
diamond and graphite
examples of CNS substances: silicon, silicon dioxide, carbon

20
Q

List the properties of covalent network substances

A

non conductors of heat and electricity in solid and liquid state **exception: graphite

extremely brittle

extremely hard

high MP and BP

insoluble in water and most other solvents

reasonably chemically inert

21
Q

Describe the bonding of covalent network substances

A

arranges in an infinite lattice structure

22
Q

explain the CNS property of electricity/heat conduction

A

non conductors: no mobile electrons because all valence electrons are tied up in covalent bonds **exception: graphite

23
Q

explain the CNS property of brittleness

A

if some bonds are broken, the rest of the lattice is placed under stress and shatters

24
Q

explain the CNS property of hardness

A

extremely hard:

breaking strong covalent bonds requires a very large amount of energy

25
Q

explain the CNS property of MP and BP

A

high MP and BP:

each atom is held in place by strong covalent bonds

breaking these bonds requires a very large amount of energy

26
Q

explain the CNS property of solubility

A

insoluble in water & most other solvents:

vary large amount of energy is required to re-arrange existing bonds in any dissolving process

27
Q

explain the CNS property of chemical inertness

A

reasonably chemically inert:

all bonding requirement are fulfilled

very large amounts of energy required to re-arrange existing bonds

28
Q

Briefly describe the structure and property of diamond

A

structure:
each carbon atoms is attached to 4 other atoms in a 3D arrangement called a tetrahedron

properties:
high MP (>3550˚C)
non conductor of electricity
brittle
extremely hard
29
Q

Briefly describe the structure and property of graphite

A

structure:
each carbon atoms is covalently bonded to 3 other atoms to form flat 2D sheets called graphene

one valence electrons from each carbon remain delocalised

properties:
high MP
good conductor of electricity
soft

30
Q

what does the mole represent in mole/mass calculations

A

measure of the number of particles in a substance

1 mole of any substance contains 6.022 x 10(23) particles

31
Q

what does molar mass represent in mole/mass calculations

A

equal to atomic, molecule and formula masses in grams

32
Q

What is mass spectrometry used for

A

determines mass and relative abundance of each isotope present in a sample of an element

33
Q

describe the process of mass spectrometry

A 
involved 4 steps:
vaporisation
ionisation
acceleration
detection
  1. sample is vaporised
  2. electrons are fired at the sample and are used to knock off electrons from the atoms, forming ions
  3. ions are accelerated and are deflected through a magnetic field (heavier ions are deflected less than lighter ions)
  4. Ions are detected and produces a mass spectrum
34
Q

list the separation techniques

A

sieving

filtration

evaporation

gravity separation

distillation

fractional distillation

35
Q

Briefly describe the separation technique of filtration

A

liquid passes through filter paper (filtrate) ad solid residue is left behind

used for:
separating very fine solid particles from liquids and gases

36
Q

Briefly describe the separation technique of sieving

A

mixture is passed through a sieve, a series of sieves may be used

based on different sizes of components, smaller particles will pass through the hole, larger particles will get caught

used for:
separating solids from liquids
e.g. straining pasta

37
Q

Briefly describe the separation technique of gravity separation

A

2 tubes containing different mixtures are spun around at a very high speed, forcing part of the mixture to settle at the bottom of the tube

used for:
separating particles from liquids
e.g. separating fat from milk

38
Q

what are the classifications of matter

A

pure substances: contain 1 type of particle

  • elements: contain 1 type of atom e.g. Ca, O2
  • compounds: contain 2 or more different types of atoms
    e. g. H2O, NaCl

mixtures: contain 2 or more different types of particles

  • homogenous
    • uniform composition
    • e.g. air, soft drinks
  • heterogenous
    • non uniform composition
    • e.g. dirty water, paints

Chemistry (8 decks)

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