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Chemistry > Topic 1 > Flashcards

Topic 1 Flashcards

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1
Q

covalent bonds

A

two non metals share a pair of electrons

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2
Q

dot and cross diagram

A

+ shows how electrons are shared
+ formula of compound can be worked out from the diagram
- makes it look like the dot and crosses are different electrons from each atom
- only shows outer electrons

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3
Q

compound

A

two or more elements/ atoms chemically bonded

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4
Q

proton

A

+1
1
nucleus

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5
Q

neutron

A

0
1
nucleus

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6
Q

electron

A

-1
1/2000
shells around nucelus

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7
Q

metals loose electrons to form

A

cations

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8
Q

non metals gain electrons to form

A

anions

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9
Q

mendeleev

A
  • arranged the periodic table by atomic number
  • left spaces for undiscovered elements
  • arranged in grouped and periods
  • metals on right and non metals on the left
  • made predictions bases on similar chemical and physical properties
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10
Q

Isotopes

A

Same atomic number but different mass number due to the number of neutrons being different

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11
Q

Ionic bond

A

Metal and non metal gain/ loose electrons

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12
Q

diatomic

A

H2
N2
O2
F2
Cl2
Br2
I2
Cl2

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13
Q

simple molecular structures

A

dont conduct electricity
low melting and boiling point

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14
Q

differences between diamond and graphite

A
  • diamond is expensive and rare
  • graphite is dull but diamond is clear
  • different lattice structures
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15
Q

similarities between diamond and graphite

A
  • made from pure carbon
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16
Q

allotropes

A

different structures made up of the same element such as diamond and graphite

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17
Q

diamond structure

A
  • consists of pure carbon with each carbon atom forming 4 covalent bonds with 4 other carbon atoms
  • giant lattice
  • high melting/ boiling point
  • very hard
  • no conductivity : no free electron
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18
Q

Graphite structure

A
  • each carbon atom covalently bonds with 3 other carbon atoms
  • the remaining electron is delocalised and is free to carry charge
    therefore can conduct electricity
  • high softness : layers can slide over each other easily as they are held by weak intermolecular forces
  • very high melting point (still a giant lattice)
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19
Q

why is diamond used for cutting tools

A

very hard

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20
Q

why is graphite used to make electrodes

A

free electrons can carry charge

21
Q

why is graphite used as a lubricant

A

the layers of carbon atoms can easily slide over each other as the intermolecular forces so little energy is needed to break them they are weak making it very slippery

22
Q

allotropes of carbon examples

A

buckminsterfullerene
C60

graphene

23
Q

diamond uses

A
  • cutting metals and glass
  • demand in jewlery
24
Q

graphite uses

A
  • pencil led
  • lubricant
  • electrodes
25
Q

graphene

A
  • one atom thick
  • strong covalent bonds
  • used in sports equipment since its light and durable
  • used in electronics
26
Q

C60

A
  • tubular or spherical
    models
  • low melting points ( weak intermolecular forces)
  • drug delivery in the body
  • simple molecule
  • hexagons and pentagons
27
Q

Nanotubes

A
  • tensile strength
  • used in nanotechnology and electronics
28
Q

polymers are made up of

A

small molecules called monomers joined together by covalent bonds

29
Q

Metallic bonding

A

The strong electrostatic attraction between a sea of delocalised electrons and a cation

30
Q

metal properties

A
  • ductile ( arranged in regular layers allowing then to slide over each other)
  • shiny
  • malleable
  • conduct electricity
31
Q

ball and stick model

A

+ shows the bonds between each atom
+ shows the 3D structure so we can see how the atoms are arranged in relation to each other
-doesn’t show teh relative sizes and distances between them
- the bonds aren’t really like sticks

32
Q

space filling model

A

+ shows 3D structure so we can see hoe atoms are arranged in relation to each other
+ more accurately represents the relative sizes and distances in relation to each other
- doesn’t show how the bonds are formed

33
Q

displayed formula

A

+ shows chemical bonds
+ formula of compound can be worked out from the diagram
- doesn’t show relative sizes or distances of atoms or bonds

34
Q

law of conservation of mass

A

mass is never lost or made in a chemical reaction in a closed system
mass of reactants = mass of products

35
Q

mr atomic or mass

A

use the MASS number

36
Q

mass of product

A
  1. check balanced
  2. known and unknown
  3. mr
  4. divide by smallest mr
  5. times by given mass
37
Q

solvent

A

something able to dissolve other substances

38
Q

solute

A

a substance that is dissolved in a solvent

39
Q

solution

A

mixture formed when solute dissolves into solvent

40
Q

concentration

A

volume of solute (g) / volume of solution (dm3)

41
Q

1dm3

A

= 1000cm3
if volume is given as cm divide by 1000

42
Q

moles

A

= mass/mr

43
Q

calculate the number of moles

A
  1. mr
  2. moles = mass/ mr
44
Q

calculate the mass of X moles

A
  1. mr
  2. number of X x mr
45
Q

shells atomic or mass

A

atomic - less

46
Q

empirical vs molecular formula

A

The empirical formula of a compound is the simplest, whole number ratio of atoms of each element in a compound.

The molecular formula shows the actual number of atoms of each element present in a compound.

47
Q

why a lid ..

A

so that no produect escapes

48
Q

why is dye used

A

makes cell more visable

49
Q

Which process moves alcohol from the blood into the liver cells?

A

diffusion

Chemistry (9 decks)

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