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Chemistry > mod 2 foundations > Flashcards

mod 2 foundations Flashcards

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1
Q

isotopes

A

same number of protons & electrons different number of neutrons

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2
Q

Relative atomic mass

A

the weighted mean mass of an element relative to 1/12 of an atom of carbon-12

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3
Q

Relative isotopic mass

A

The mass of an atom of isotope compared with 1/12 of the mass of an atom of carbon-12

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4
Q

Calculate RAM

A

(% x mass) + (% x mass)

100

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5
Q

Moles

A

The amount of substance that contains 6.02 x 10^23 of particles same as 12g of carbon-12

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6
Q

avogadros constant

A

6.022 x 10^23

N= n x NA

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7
Q

Ideal gas law

A 
PV = nRT
P=pressure (pa)
V=volume(m3)
R=constant(8.31)
T=temp (k)
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8
Q

properties of ideal gas law

A
  • all particles are identical & in random continuous motion
  • particles travel in straight lines
  • the particles dont react when they collide
  • the particles have no intermolecular forces between them
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9
Q

Molar gas volume

A

At room temp and pressure, 1 mole of gas occupies a volume of 24dm3
V= n x 24dm3

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10
Q

Percentage yield

A

actual yield / theoretical yield

x100

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11
Q

Atom economy

A

Mr of desired product / sum of all Mr of reactants

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12
Q

Water of crystalisation

A

Water molecules that form part of the crystalline structure
anhydrous-dehydrated (no water)
hydrated(water)

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13
Q

metallic bonding

A

strong electrostatic force of attraction between positively charged ions and sea of delocalised electrons

  • high melting and boiling points
  • good conductors (solid&liquid)
  • malleable&ductile
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14
Q

covalent bonding

A

strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atom
eg-N2,CO2

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15
Q

Dative covalent bond

A

one element gives both electrons to the bond

eg-NH4

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16
Q

Ionic bonding

A

electrostatic attraction between positive & negative ions
-metal&non metal
-giant lattices
higher the charge the stronger the bond

17
Q

general equations

A

Acid + metal = salt + hydrogen
Acid + base =salt +water
Acid + metal carbonate= salt+ water+ carbon dioxide

18
Q

Oxidation state

A

tells us the charge of an element, indication of how many electrons an element has lost or gained

19
Q

oxidation state rules

A

-all elements in their uncombined state has an oxidation state of 0
-oxygen normally -2
cl is different if binded with fluorine or oxygen
-hydrogen have +1 unless bonded to metal -1

20
Q

bases

A

substances that can react with an acid to forma salt

  • sodium hydroxide (NaOH)
  • potassium hydroxide(KOH)
  • ammonia- (NH3)
21
Q

electron shells

A

2,8,18,32
s=2, p=6, d=10 f=14
1s,2s,2p,3s,3p,4s,3d etc

22
Q

orbitals

A 
s-orbitals 
sphere shape
p orbitals
-dumbell shape (3 kinds)
each orbital hold 2 electrons so therefore in p shell there are 3 orbital shells
23
Q

short hand notation

A

write the nearest noble gas in square brackets then write the continuing shells

24
Q

electron configuration

A

-draw with single headed arrows
opposite way to eachother as electrons repel
-put electrons in each box before filling each pair out
most stable if half full or full

25
Q

shapes of molecules

A 
linear = 180 (co2)
triganal planar = 120 (BCl3)
tetrahedral = 109.5 (CH4)
pyramidal = 107 (NH3)
non-linear = 104.5 (H2O)
octahedral = 90 (SF6)
-lone pairs repel more than bonded
26
Q

electronegativity

A

-an atoms ability to attract bonding electrons in a bond
-measured using pauling scale
-Across periodic table; electronegativity increases,nuclear charge increases, ar decreases
less than 0.5 = non polar
0.5 - 1.8 = polar
bigger than 1.8 = ionic

27
Q

Bond polarity

A

non polar- if elements are similar in electronegativity or the same eg H2
polar- if electronegativities are different eg HCl
separation of opposite charges (dipoles)
Solvents dissolve in like substances
polar dissolves in polar

28
Q

intermolecular forces

A 
induced dipole (london forces) - weak forces that exist between all molecules; electrons move to one side causing a temporary charge
permanent dipole -  stronger than london; exist in polar covalent bonds
hydrogen - strongest force; dipole bonds with lone pair, between H-N,F,O
29
Q

Anomolous water properties

A

ice is less dense than water - hydrogen bonds hold water molecules apart in a lattice

  • water has relatively high boiling point
  • high surface tension
30
Q

empirical formula

A

simplist whole number ratio
-work out number of moles of each then divide by smallest number of moles
will give you a ratio then round to nearest whole number

31
Q

uncertainty

A

% = (2x) uncertainty / quantity measured
x100
-(2x) if using a burette as there are 2 uncertainties

32
Q

compound charges

A 
sulphate - SO4 (2-)
nitrate - NO3 (-)
carbonate CO3 (2-)
hydroxide OH (-)
ammonium NH4 (+)

Chemistry (9 decks)

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