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Chemistry IGCSE > Chapter 2 > Flashcards

Chapter 2 Flashcards

1
Q

Elements

A

Consits of one type of atom only

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2
Q

Compunds

A

Made up of two or more different elements which are chemically bonded together -> properties of compound differ from properties of original elements + difficult to seperate

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3
Q

Mixtures

A

Made up of two or more elements or compunds that aren’t chemically bonded together -> properties of mixture: a mixture of the properties of seperate parts + easily seperated with pysical methods

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4
Q

Atomic structure

A

Central nucleus containing protons and neutrons surrounded by electrons in shells

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5
Q

Neutral atoms

A

No overall charge as number of protons is equal to number of electrons -> if some electrons are added or removed the atom becomes charged and is now an ion

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6
Q

Relative mass of proton

A

1

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7
Q

Relative mass of neutron

A

1

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8
Q

Relative mass of electron

A

Approx 0 -> 0.0005

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9
Q

Relative charge of proton

A

+1

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10
Q

Relative charge of neutron

A

0

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11
Q

Relative charge of electron

A

-1

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12
Q

Atomic number/ proton number

A

Number of protons in nucleus of atom -> in neutral atom this tells us the element
(Smaller number)

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13
Q

Mass number/nucleon number

A

Number of protons and neutrons in nucleus of atom
(Bigger number)

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14
Q

Isotopes

A

Different atoms of the same element that have the same number of protons but different number of neutrons
- Isotopes have the same chemical properties, as chemical properties depend on the number of electrons and isotopes have the same number of electrons/electronic configuration

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15
Q

Relative atomic mass of an element (Ar)

A

Average mass of all isotopes of the element

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16
Q

Electron shell rules

A
  • Electrons always occupy shells (energy levels)
  • Lowest shells always filled first -> shells closest to nucleus
  • Certain capacity of electrons in each shell
17
Q

1st shell

A

2 electrons

18
Q

2nd and 3rd shell

A

8

19
Q

Outer shell electrons

A

Control reactivity as they from bonds with other atoms to gain or loose enough electrons to achieve a full outer shell and become stable + unreative

20
Q

Ions

A

Charged particles

21
Q

Anions

A

Negative ions -> form when atoms gain electroms

22
Q

Cations

A

Positive ions-> form when atoms loose electrons

23
Q

Ionic bonding

A

Between metals and non-metals -> metal atom looses electrons to form a cation and a nonmetal gains these electrons to form an anion
- These oppositely charged ions are strongly attracted to each other by electrostatic attractions -> ionic bonding

24
Q

Ionic compund properties

A

Always have gaint ionic structure -> regular arrangement of alternating positive and negative ions
- High melting/boiling points (low volatility) -> strong attractive forces between closely packed ions in giant ionic lattice (takes a lot of energy no break bonds)
- When solid -> can’t conduct electricty but do conduct when aqueous or molten -> ions are mobile and carry electric charge

25
Q

Covalent bond

A

Pair of electrons shared between two atoms to a noble gas electron configuration

26
Q

Covalent compund properties

A
  • Low melting/boiling points (high volatility) -> intermolecular forces are weak
  • Don’t conduct electricty -> don’t have ions, only uncharged molecules
27
Q

The 3 types of giant covalent structures

A

Graphite
Diamond
Silicon

28
Q

Graphite: description

A
  • Black, shiny solid
  • Each carbon atom forms 3 covalent bonds -> sheets of carbon atoms arranged in hexagons
29
Q

Graphite: properties

A
  • High melting/boiling point -> covalent bonds in hexagon need loads of energy to break
  • Conducts electricity -> each carbon atom has one electron that’s delocalised which can move and carry electric charge: Graphite often used for electrodes
  • No covalent bonds between layers so they can slide over eachother -> this makes graphite soft and slippery: graphite used as lubricant material
30
Q

Diamond: description

A
  • Transparent colourless crystals
  • Each carbon atom forms four covalent bonds -> tetrahedral structure formed
31
Q

Diamond: properties

A
  • High melting/boiling point -> strong covalent bonds need lots of energy to break
  • Very hard-> covalent bonds hold atoms in rigid lattice structure: Diamond used as cutting tool
  • Doesn’t conduct electricity -> no free electrons
32
Q

Silicon (IV): Description

A
  • Similar giant tetrahedral lattice to diamond
  • Silicon atoms positioned like carbon atoms in diamons, with an oxygen atom between each one
33
Q

Silicon (IV): properties

A
  • High melting/boiling point -> strong covalent bonds need loads of energy to break
  • Hard -> covalent bonds hold atoms in rigid lattice structure
  • Doesn’t conduct electricity -> no free electrons
34
Q

Metallic bonding

A

Electrostatic attraction between the positive ions in a giant metallic lattice and a ‘sea’ of delocolised electrons which holds atoms together in a regular structure

35
Q

Physical properties of metallic bonding

A
  • Good electrical conductivity: delocolised electrons are free to move and carry electric charge
  • Ductility and malleability: positive ions in metal arranged regularly in layers, when force applied layers can slide over ecah other
36
Q

Giant ionic lattice

A

Regular arrangement of alternating positive and negative ions

Chemistry IGCSE (11 decks)

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