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GENERAL IGCSE Chemistry > Atoms, elements and compounds > Flashcards

Atoms, elements and compounds Flashcards

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1
Q

What is the mass and charge of a proton?

A

Mass: 1 unit
Charge: +1

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2
Q

What is the mass and charge of a neutron?

A

Mass: 1 unit
Charge: no charge

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3
Q

What is the charge of an electron?

A

Charge: -1

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4
Q

What is the proton number/atomic number?

A

number of protons in nucleus of atom

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5
Q

What is the nucleon number?

A

number of protons and neutrons in the nucleus of an atom/relative atomic mass

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6
Q

What do columns in a periodic table show?

A

groups with similar reaction properties

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7
Q

What do rows in a periodic table show?

A

periods

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8
Q

What are isotopes?

A

atoms of same element with same proton number, different number of neutrons → different nucleon number

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9
Q

Why do isotopes have the same properties?

A

same properties because same number of electrons in outer shell

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10
Q

What are the two types of isotopes?

A

radioactive

non-radioactive

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11
Q

What are some medical and industrial uses for radioactive isotopes?

A

Medical: cancer treatment, locating tumours
Industrial: check for oil and gas leaks

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12
Q

What is oxidation state/valency number?

A

number of electrons in outer shell

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13
Q

Why is group 0 unreactive?

A

full outershell

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14
Q

Why do atoms with more electron shells have higher energy levels?

A

Further away from nucleus

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15
Q

What is an ion?

A

electrically charged particle

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16
Q

What is an ionic bond made of?

A

Metals + Non-metals

17
Q

How are ionic bonds formed?

A

Atoms lose/gains electrons to become stable

18
Q

What is the structure of ionic bonds?

A

arranged in a giant lattice with regular pattern of particles held together by strong ionic bonds

19
Q

What are the properties of ionic compounds (5)?

A

High boiling + melting points (ionic bonds strong)
Poor conductors as solid (no free electrons/ions)
Conducts electricity as liquid
Hard
Soluble in water

20
Q

Why do ionic compounds have high fixed points?

A

ionic bonds strong, lots of energy required to overcome electrostatic attraction

21
Q

Why do ionic compounds conduct electricity as liquid?

A

charged ions free to move

22
Q

What is a covalent bond made of?

A

Non-metal + Non-metal

23
Q

What are molecules?

A

a group of atoms held together by COVALENT bonds

24
Q

How are covalent bonds formed?

A

Atoms share pairs of electrons to achieve noble gas configuration

25
Q

What is the strength of bonding in covalent bonds ?

A

Molecular bonds strong, intermolecular are weak

26
Q

What are the properties of covalent compounds?

A

Low melting/boiling points
Don’t conduct electricity (not charged)
Insoluble in water, but dissolve in organic solvents

27
Q

Why do covalent compounds have low fixed points?

A

weak intermolecular forces

28
Q

How many electrons are shared in a single, double and triple covalent bond?

A

Single bond: 2 electrons shared (1 from each atom)
Double bond: 4 electrons shared (2 from each atom)
Triple bond: 6 electrons shared (3 from each atom)

29
Q

Why do giant covalent structures have high fixed points?

A

structure made up of strong covalent bonds

30
Q

Why don’t giant covalent structures conduct electricity?

A

have no mobile ions or electrons, except for graphite

31
Q

What are the properties of diamond? (4)

A

Shares 4 valence electrons → 3D lattice
Strong covalent bonds
High fixed points
Forms tetrahedron

32
Q

What are the properties of graphite? (6)

A

Shares 3 valence electrons
4th electron free – Free moving electrons
Strong covalent bonds
Held together by weak forces so is soft and slippery -used as a lubricant
Slide over each other

33
Q

What are the properties of silicon dioxide? (5)

A 
Makes up sand  
Each Si is bonded to 4 oxygen atoms
Each oxygen bonded to 2 silicon atoms  
High fixed points  
Hard
34
Q

What are delocalized electrons

A

Free electrons in metallic bonding

35
Q

Why can metals conduct electricity and heat?

A

Delocalized electrons can carry charge

36
Q

Why are metals malleable + ductile?

A

attractive forces between metal ions and electrons act in any direction – when layers slide new bonds can easily form

GENERAL IGCSE Chemistry (22 decks)

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