Brainscape's Knowledge GenomeTM

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


See full index

Chemistry Daisy > Key Terms In Chemistry > Flashcards

Key Terms In Chemistry Flashcards

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

JJ Thompson’s Plum Pudding Theory

A

Positively charged sphere

With electrons that are negatively charged atoms

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

Rutherfords Model

A

Tiny positively charged nucleus at the centre
Surrounded by a cloud of negative electrons
Most of the atom is empty space

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

Gold Leaf Test - Rutherford

A

Fired positively charged alpha particles at a thin gold sheet.
Most particles went straight through, some were deflected and a small number were backwards- so the plum pudding could not be right

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

Bohr’s Model

A

Electrons only exist in fixed orbits or shells

Each shell has a fixed energy

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

Protons

  • relative mass
  • relative charge
A

Heavy and positively charged
Relative Mass - 1
Relative Charge - +1
Found in the nucleus which is positively charged

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

Neutrons

A 
Heavy
Neutral 
Relative mass - 1
Relative charge - 0
Found in nucleus
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Electrons

A

Negative
Relative mass- 0.0005
Relative Charge - -1
Found in electron shells

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

Atomic number

A

Tells you how many protons and electrons there are in the atom

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

Mass number

A

Tells you the total number of protons and neutrons in an atom

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

Isotopes

A

Different forms of the same element, which have the same number of protons but a different number of neutrons.

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

How do you calculate the relative atomic mass from isotopic abundances?

A

Multiply each relative atomic mass by its isotopic abundance and add up the results
Divide by the sum of the abundance’s

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

How did the order of the periodic table come about?

A

Dmitri Mendeleev arranged them based on their properties, then realised they were in order of atomic mass

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

What do periods show in the periodic table?

A

Represent a new full shell of electrons

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

What do groups show on the periodic table?

A

Corresponds to the number of electrons it has on its outer shell

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

Ions

A

Ions are charged particles- when atoms lose or gain electrons to form ions

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

When do negative atoms form?

A

Anions - when atoms gain electrons- they have more electrons than protons so they are negatively charged

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

When do positive ions form?

A

Cations- when atoms lose electrons - they have more protons than electrons - they are positively charged

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

Group 1 and 2 ions

A

They are metals so they lose electrons to form positive ions

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

Group 6 and 7 ions

A

Non metals that gain electrons to form negative ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Ionic bonding

A

When a metal and non metal react together

  • the metal atoms loses electrons to form a positive ion
  • the non metal gains these to form a negative ion
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What are oppositely charged ions attracted to each other by?

A

They are strongly attracted to one another by electrostatic forces this is called an ionic bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Ionic compound shapes

A

Always have a giant ionic lattice structures. The ions form a closely packed regular lattice
There are very strong electrostatic forces of attraction between oppositely charged ions in all directions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Ionic compound properties

-melting and boiling points

A

High melting and boiling points due to the strong attraction between the ions. It takes a large amount of energy to overcome this attraction.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Ionic compound properties

-conductor of electricity?

A

Solid ionic compounds don’t conduct electricity because the ions are in a fixed place and can’t move.
But when an ionic compound melts, the ions are free to move and can carry an electric current.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Ionic compound properties

- dissolvable?

A

Many dissolve easily in water. The ions separate and are all free to move in the solution- so they’ll carry and electric current.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Advantages of models that show ionic compound structures

A

2D representations of molecules are simple and great at showing what atoms contain and how they are connected.
Dot and cross diagrams- show how compounds are formed
3D models show the arrangement of ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Disadvantages of models that show the structure of ionic compounds

A

2D representations don’t show the shape of the substance or the size of atoms
Dot and cross diagrams don’t show the size or how they are arranged
3D models only show the outer layer of the substance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Covalent Bonding

A

Is a strong bond that forms when a pair of electrons is shared between two atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

What are simple molecular substances made up of?

A

They are made up of molecules containing few atoms joined by covalent bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

Properties of simple molecular substances

  • bonds
  • forces of attraction
A

Atoms are held together by very strong covalent bonds

The forces of attraction are very weak

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Properties of simple molecular substances

  • melting and boiling points
  • what substance are they at room temperature?
A

To melt or boil, you only need to break the weak intermolecular forces - melting and boiling points are very low
Most molecular substances are liquid or gas at room temp

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

Properties of simple molecular substances

  • the bigger the molecules the…?
  • conducts electricity?
A

As molecules get bigger, the strength of the intermolecular forces increases, so more energy is needed to break them - melting and boiling points increase
-don’t conduct electricity as they don’t contain any free electrons or ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

Polymers

How are they formed?

A

Are molecules made up of long chains of covalently bonded carbon atoms
-they are formed when lots of small molecules called monomers join together

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

Giant covalent structure properties

  • bonds
  • melting and boiling points
A

All atoms are bonded together by strong covalent bonds

Very high melting and boiling points as lots of energy is needed to break the covalent bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

Giant covalent structure properties

  • conductor of electricity?
  • soluble?
A

Don’t contain charged particles - don’t conduct electricity

Aren’t soluble in water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

Diamond - giant covalent structure

  • how many covalent bonds?
  • melting points?
A

Made up of a network of carbon atoms that each form four covalent bonds
Strong covalent bonds take lots of energy to break- high melting point

37
Q

Diamond - giant covalent structure

  • lattice structure
  • conductor of electricity?
A

Strong covalent bonds hold the atoms in a rigid lattice structure- making diamonds really hard
Doesn’t conduct electricity - no free electrons or ions

38
Q

Graphite - Giant covalent structures

  • how many covalent bonds?
  • how strong are the layers?
  • what properties does graphite have?
A

Each carbon atoms forms three covalent bonds- creating sheets of carbon atoms arranged in hexagons
No covalent bonds between layers- weakly held together so they are free to move over each other
- this makes graphite soft and slippery

39
Q

What is diamond used for?

A

Used to strengthen cutting tools- as it is really hard as it has a rigid lattice structure

40
Q

What is graphite used for?

A

Lubricating material as it’s soft and slippery as the layers can move over each other

41
Q

Graphite- giant covalent structures

  • melting points
  • conductor of electricity?
A

High melting point - covalent bonds need lots of energy to break
Only three out of carbons four electrons are used in bonds- so each carbon atom has one delocalised electron and can move.
- so it conducts electricity

42
Q

Graphene- giant covalent structure

  • what is it?
  • how many atoms thick?
A

A type of fullerene- one layer of graphite
Sheet of carbons are joined to together in hexagons
Sheet is one atom thick- making 2 dimensional

43
Q

Fullerenes

A

Are molecules of carbon shaped like closed tubes or hollow balls

44
Q

What are fullerenes made up of?

A

Carbon atoms arranged in hexagons

45
Q

What are fullerenes used for?

A

Can be used to cage other molecules. Fullerenes structure forms around another atom or molecule which is then trapped inside.
This could be used to deliver a drug directly to cells in the body

46
Q

How could fullerenes large surface area help?

A

They could help make a great industrial catalysts - individual catalyst molecules could be attached to the fullerenes

47
Q

What is metallic bonding?

A

Electrons in the outer shell of metal atoms are delocalised. There are strong forces of electrostatic attraction between the positive ions and the shared negative electrons

48
Q

What do the forces of attraction do? Metallic bonding

A

They hold the atoms together in a regular structure and are known as metallic bonding

49
Q

What are metals physical properties?

-melting and boiling points

A

Electrostatic forces between the metal ions and delocalised sea of electrons are very strong, so need lots of energy.
High melting and boiling points - metals are generally shiny

50
Q

What are metals physical properties?

-dense?

A

Metals are more dense as ions in the metallic structure are packed closely together.

51
Q

What are some physical properties of metals?

- malleable?

A

Malleable - layers of atom in a pure metal can slide over each other- they can be hammered or rolled into small sheets

52
Q

What are some physical properties of metals?

-conductor of electricity and heat?

A

The delocalised electrons carry electrical current and thermal energy through the material- so metals are good conductors of heat and electricity

53
Q

Dot and cross diagram

A

Is used to explain what happens when a bond is formed. It uses dots and crosses to represent the electrons in different atoms

54
Q

Properties of simple molecular structures - covalent

A

Simple molecules
Low melting and boiling points
Some are soluble
Don’t conduct electricity

55
Q

Monomers

A

Small , simple molecules that can be joined to make polymers

56
Q

Properties of monomers

A

Small chain
Small forces
Low energy
Low melting points

57
Q

Properties of polymers

A

More forces
Long chain
More energy
High melting points

58
Q

Allotropes

A

Are different structural forms of the same element

59
Q

Properties of non metals

A

Insulators
Liquids, gas and solids
Low and high melting points
Brittle

60
Q

Why are metals malleable?

A

Force is applied to metals, the regularly arranged ions are free to move over one another. Ions are still held together by delocalised electrons so they do not break

61
Q

Why do metals conduct electricity?

A

The delocalised electrons are free to move. This means when a potential difference is applied, the electrons flow in one direction.

62
Q

Symbol equations must always be…

A

Balanced and there must always be the same number of atoms of each element on both sides of the equation.

63
Q

State symbol (s)

A

Solid

64
Q

State symbol (l)

A

Liquid

65
Q

State symbol (g)

A

Gas

66
Q

State symbol (aq)

A

Aqueous

67
Q

What does aqueous mean?

A

Dissolved in water

68
Q

Formula for water

A

H20

69
Q

Formula for carbon dioxide

A

CO2

70
Q

Formula for ammonia

A

NH3

71
Q

Formula for hydrogen

A

H2

72
Q

Formula for chlorine

A

Cl2

73
Q

Formula for oxygen

A

O2

74
Q

Formula for ion ammonia

A

NH+

4

75
Q

Formula for hydroxide ion

A

OH-

76
Q

Formula for ion nitrate

A

NO-

3

77
Q

Formula for carbonate ion

A

CO. 2-

3

78
Q

Formula for sulfate ion

A

SO. 2-

4

79
Q

Ionic equations method

A

Look at the balanced equation
Any ions or aqueous things break up into ions
Take out any aqueous ions that are present on both sides of the equation

80
Q

Oxidising

A

Provides oxygen which allows other materials to burn more fiercely

81
Q

Environmental hazard

A

Harmful to organisms and the environment

82
Q

Toxic

A

Can cause death if swallowed, breathes in or absorbed by skin

83
Q

Harmful

A

Can cause irritation, reddening of the skin and blistering

84
Q

Flammable

A

Catches fire easily

85
Q

Corrosive

A

Destroys materials inc,using living tissues

86
Q

Steps for risk assessment questions

A

State the hazard symbol each chemical is
Explain what it means
Explains ways to reduce risk

87
Q

What was different about how Mendeleev thought he arranged the periodic table?

A

He thought he has arranged elements in order of increasing relative atomic mass but this was not always true because of the relative abundance’s of isotopes of some pairs of elements in the periodic table

88
Q

What are elements in the same columns?

A

Similar properties

89
Q

What are elements placed in rows?

A

In atomic order

Chemistry Daisy (6 decks)

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