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nat 5 chem > unit 1 > Flashcards

unit 1 Flashcards

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1
Q

Factors affecting rate of reaction

A

PARTICLE SIZE- increase in particle size=decrease in rate
CONCENTRATION- increase=more present particles=more likely collisions
TEMPERATURE- increase=particles more energy, move faster, more likely collisions
CATALYST USE- speed up reactions without being used up

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2
Q

Av Rate of Reaction Calculation

A

Δreactant/product ÷ Δtime

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3
Q

Periodic Groups

A

1=ALKALI METALS- very reactive metals
0=NOBLE GASES- unreactive
7=HALOGENS- very reactive non-metals

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4
Q

Nuclide Notation

A

MASS NO.- protons+neutrons

ATOMIC NO. - protons (also no. of electrons-atoms r neutral)

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5
Q

similar chemical properties

A

elements in same group have similar them properties as have same no. of outer electrons

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6
Q

Isotopes

A

Atoms which have SAME ATOMIC NO. but DIFFERENT MASS NO.

no. of NEUTRONS differs

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7
Q

Relative Atomic Mass

A

R.A.M of element = av mass element -Takes into account MASS of each isotope &PROPORTION of each isotope

R.A.M value- CLOSEST to MASS of most ABUNDANT isotope

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8
Q

Ions

A

ion is a charged particle formed by loss/gain of electrons

electron loss/gain diagram [ ]

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9
Q

What is the charge of ions depending on the group

A

Group 1 2 3 4 5 6 7 8
Charge + + 2 + 3 / 3- 2- - /

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10
Q

Ion-electron Equation (formation of ion)

A

S+ + 2e- → S2-

element - how much loss/ gain e - produces - Ion

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11
Q

Flame Testing

A

Flame test is analytical procedure used to detect presence of certain elements, primarily metal ions, based on color produced during test

many metal ions burn w coloured flames

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12
Q

How to test for element

A
  • flame testing
  • does element conduct
  • what temp it melts/boils at
  • H burns w squeaky pop, CO2 turns lime water cloudy
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13
Q

Bonding

A
  1. tranferring electrons - FORM IONS

2. share electrons - COVALENT BONDS

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14
Q

Ionic bonding

A

IONIC BONDS R ELECTROSTATIC FORCE OF ATTRACTION BETWEEN + AND - IONS

  • metal bonds to nonmetal atom
  • metal becomes +charge, nonmetal becomes -charge
  • as 2 particles oppositely charged become attracted, form ionic bond

Ionic bonding diagram [ ]

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15
Q

what is the structure of Ionic Crystal Lattices [Ionic Compounds]

A

Ionic compounds form lattice structures of oppositely charged ions w each +ion surrounded by -ions, vice versa

ionic bonds r so strong- ions r fixed together unable to move

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16
Q

Formula of ionic Compound

A

tells Ratio of ions in lattice, not actual no. of ions present:

            Ca  :    F ratio:          1   :   2

formula: CaF₂

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17
Q

Covalent bonding

A

FORCES OF ATTRACTION MADE BY NONMETAL ATOMS SHARING OUTER ELECTRONS. molecule is group atoms held together by covalent bonds.

Bonding(e sharing) diagram

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18
Q

What holds atoms together?

A

NUCLEI of atoms have MUTUAL ATTRACTIONS FOR SHARED PAIR OF ELECTRONS.

this holds atoms together in covalent bonds

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19
Q

what are Diatomic elements and name them

A

diatomic molecule only has 2 atoms

H2, N2, I2, Br2, F2, O2, Cl2

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20
Q

Shapes of Molecules

A
  1. LINEAR
  2. ANGULAR
  3. TRIGONAL PYRAMIDAL
  4. TETRAHEDRAL
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21
Q

Covalent Network Structures

A

billions atoms in one crystal joined together as one giant molecule- network structure e.g. carbon in form of graphite/diamond, silica(sand)

covalent substances can either form discrete(small molecule) molecular subs/giant network structures

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22
Q

Metallic Bonding

A

Metallic bonding is ELECTROSTATIC FORCE OF ATTRACTION BETWEEN POSITIVELY CHARGED IONS AND DELOCALISED ELECTRONS

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23
Q

how are Metallic Structures made

A

consists of one giant lattice of +charged ions in sea of delocalised outer electrons.- free to move.

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24
Q

Melting and Boiling Point of Covalent Molecular Structures

A

To move molecules apart forces of attraction between molecules must be broken

C.M.S. FORCES R WEAK- tend to have LOW MELTING & BOILING POINTS

as result most r GASES/LIQUIDS at room temp

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25
Q

Melting and Boiling Points of Covalent Network Structures

A

MELTING involves BREAKING STRONG COVALENT BONDS within networks

REQUIRES LOT OF ENERGY- MELTING & BOILING POINTS R HIGH

26
Q

Melting and Boiling Points of Ionic Substances

A

MELTING involves BREAKING STRONG IONIC BONDS between ions in lattice

REQUIRES LOT OF ENERGY- HIGH MELTING & BOILING POINTS

27
Q

Solubility of ionic substances in water and do covalent substances dissolve in water

A

WATER GOOD for many IONIC SUBS. [ LATTICE BREAKS UP COMPLETELY TO LEAVE MANY FREE IONS IN SOLUTION ]

MOST COVALENT SUBS DONT DISOLVE IN WATER BUT CAN IN OTHER SOLVENTS

28
Q

Conductivity in Elements

might need diagram

A
  • METAL elements CONDUCT

- NONMETAL DONT- exception is CARBON in form GRAPHITE

29
Q

Conductivity in Compounds

might need diagram

A
  • COVALENT SUBS DONT CONDUCT in any state

- IONIC SUBS CANT CONDUCT SOLID, CAN IN SOLUTION/MOLTEN

30
Q

Electricity

A

a flow of charged particles

31
Q

Conductivity in Metallic Bonding

A

all metals can conduct as delocalised electrons are free to move

32
Q

Conductivity in Covalent Bonding

A

Covalent subs don’t conduction any state as there’s no charged particles free to move

33
Q

Conductivity in Ionic Bonding

A

solid- don’t conduct as ions held tight in lattice and aren’t free to move

dissolved in water/molten- ionic lattice breaks up completely and ions free to move

34
Q

electrolysis

A

an ionic solution or melt which conducts electricity-called an ELECTROLYTE
Process of passing current through electrolyte- ELECTROLYSIS

ELECTROLYSIS= splitting compound into constituent elements. D.C. power supply used to identify products

35
Q

what happens during Electrolysis

might need diagram

A

During electrolysis:
+METAL IONS attracted to -ELECTRODE where they GAIN electrons

-NONMETAL IONS attracted to +ELECTRODE where they LOSE electrons

36
Q

Formula for Compounds

A

ide- contain 2 elements

ite/ate- oxygen is present

37
Q

Valency

A

Combining power of element is no. of single bonds it can make

Group 1 2 3 4 5 6 7 8
valency 1 2 3 4 3 2 1 0

38
Q

formula mass calculations

A

m n gfm

39
Q

calculations based equations

A

in question mentions 2 subs
needs balanced equation
use molar ratio
m n gfm & n c v

40
Q

n=cv units

A

c=mol/l or mol l-1
v= litres (remember to CONVERT if in CM3)
n=moles

41
Q

What is a Solution

A

SOLUTION when SOLUTE(SOLID) dissolves in SOLVENT(LIQUID)

42
Q

Standard Solutions

A

A SOLUTION whose CONCENTRATION is ACCURATELY KNOWN

cld have to do molar ratio qs

43
Q

How to Make Standard Solution

A
  • CORRECT MASS OF SUBSTANCE ACCURATELY MEASURED (beaker/weighing boat)
  • ALL SUCCESSFULY TRANSFERRED TO VOLUMETRIC FLASK
  • TAKE A RINSING of whatever was used to measure substance
  • KEEP ADDING WATER TO FLASK TILL BOTTOM OF MENISCUS TOUCHES THE MARK
44
Q

What is pH scale indication of

A

the hydrogen ion concentration of a solution

45
Q

why is water neutral

A

-DISASSOCIATES into equal concentration of H+and OH- ions
-REVERSIBLE REACTION
only small amount disassociate

46
Q 
Acid solution formula of:
Hydrochloric acid 
nitric acid
Sulphuric acid
Ethnoic acid
A

HCL
HNO3
H2SO4
CH3COOH

47
Q 
Alkali solution formula of:
Sodium hydroxide 
Potassium hydroxide
Calcium hydroxide 
Ammonia
A

NaOH
KOH
Ca(OH)2
NH3

48
Q

What happens to acid/alkali when diluted

A

pH no. moves toward 7

49
Q

how to make Alkali solution

A

METAL OXIDES & HYDROXIDES DISSOLVED IN WATER = ALKALINE SOLUTION

Ammonia gas dissolved in water= alkali

50
Q

how to make an acid

A

NON METAL OXIDES DISSOLVED IN WATER= ACIDIC SOLUTION

51
Q

what affect do insoluble substances have on pH of water

A

insoluble subs do not affect pH of water

52
Q

What is a Base

A

BASE= substance which NEUTRALISES ACID

BASES= METAL OXIDES, METAL HYDROXIDES, METAL CARBONATES

Alkalis r bases that dissolve in water(soluble bases)

53
Q

What is Neutralisation

A
  • REACTION of ACID W ALKALI
  • Produces SALT & WATER
  • When base is METAL CARBONATE CO2 formed too
54
Q

What are Volumetric Titrations

A

Technique that allows EXACT ACID VOLUME NEEDED to NEUTRALISE ALKALI to be CALCULATED

55
Q

How to do Titration

A
  • burette filled w acid up to 0 mark
  • u know ACID CONC but not of ALKALI
  • KNOWN V of ALKALI put in conical flask-contains INDICATOR
  • acid carefully let into flask
  • when ALKALI NEUTRALISED, indictor changes colour, stop acid flow= ENDPOINT
56
Q

For how long is Titration Repeated Till

A

till 2 CONCORDANT(lie within .2cm3) RESULTS OBTAINED

57
Q

How do you do a volumetric titration calculation

A
  • Rough titration ignored
  • calc av of concordant results (Volume)
  • do molar ratio equation calc using n,c,v
58
Q

What is a precipitation reaction

A

when 2 SOLUTIONS REACT TO FORM A SOLID (called PRECIPITATE)

SOLID CAN BE COLLECTED BY FILTRATION

59
Q

How can a Precipitation Reaction be Easily Identified

A

by the formation of a Solid product from Aqueous Reactants

60
Q

How do you do Ionic Equations

Precipitation reactions-making insoluble salts

A
  1. write out BALANCED EQUATION W STATE SYMBOLS
  2. SPLIT ionic compounds writing in individual CHARGES & any small no.’s outside brackets make them big in front. Remove state symbols
  3. in same line SCORE OUT SPECTATOR IONS
  4. write out what’s left of ionic equation
61
Q

What are Spectator Ions

A

ions which remain UNCHANGED by reaction as they DONT TAKE PART in REACTION

62
Q

Drawing Line Graph tips

important

A
  • unlike in biology always FREEHAND graphs
  • line/curve is for GENERAL TREND
  • LINE DOESNT NEED TO PASS EVERY POINT; outlier/error
  • for curved line freehand, doesn’t need to pass each point
  • for straight line use ruler, doest need to pass each point

nat 5 chem (2 decks)

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