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IGCSE Chemistry > C3 - Atoms, Elements and compounds > Flashcards

C3 - Atoms, Elements and compounds Flashcards

1
Q

An atom is made up of a

A

positively charged nucleus surrounded by negatively charged electrons

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2
Q

The atomic number is the number of

A

protons in an atom of a particular element

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3
Q

The mass number of an atom is

A

the number of protons and neutrons found in a nucleus

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4
Q

What is the mass and atomic number of sodium

A

Mass number = 23

Atomic number = 11

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5
Q

What sub atomic particles make up the nucleus

A

protons and neutrons

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6
Q

Difference between physical and chemical changes

A

Physical changes change the appearance of a substance and not the chemical composition whilst in a chemical change one or more new substances are produced.

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7
Q

What experiment shows that some chemical changes can be reversed

A

Hydrated blue copper sulfate crystal test
When heated a white powder will form (anhydrous copper sulfate) and water is lost as steam. If water is added it turns blue.

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8
Q

What is the relative mass of protons, neutrons and electrons

A 
proton = 1
neutron = 1
electron = 1/2000
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9
Q

Another name for mass and atomic number

A

nucleon number (for mass) and proton number (for atomic)

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10
Q

Hydrogen has a proton and electron but no

A

neutron

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11
Q

In an atom the number of protons is equal to the

A

number of electrons

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12
Q

In a periodic table the elements are arranged via

A

their atomic number

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13
Q

Atoms have no

A

overall charge

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14
Q

When an atom becomes charged due to losing or gaining electrons it is called an

A

ion

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15
Q

If atoms lose one or more electrons in outer shell its called a

A

positive ion

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16
Q

If an atom gains one or more electron in outer shell its called a

A

negative ion

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17
Q

What is an isotope

A

A same element atom with same number of protons but different number of neutrons

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18
Q

Isotopes have the same properties as their regular atoms because

A

they have the same number of electrons in the outer shell

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19
Q

A nuclide is a

A

type of isotope that is characterized due to its distinct specific nucleus

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20
Q

Electrons have fixed positions in atoms called

A

electron shells

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21
Q

What is the electron configuration of an atom

A

2 electrons max on the first shell

then it’s 8 max on the next shell after that.

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22
Q

The closer a shell is to the nucleus of an atom

A

the lower its energy level is

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23
Q

What is the electron configuration of an atom of sodium

A

11 electrons in sodium so

2,8,1

24
Q

What is an ionic bond between

A

a metal (+) and a non-metal (-)

25
Both metals and non-metals try to achieve a
complete outer electron shell
26
Properties of non-metals
``` Poor conductors of electricity Low melting and boiling points Dull Brittle Poor conductors of heat ```
27
Ionic bonding involves the
attraction between two oppositely charged ions to achieve a full outer shell of electrons
28
What are the 3 ways atoms can be chemically bonded
Ionic bonding, covalent bonding and metallic bonding
29
Covalent bonding involves bonding between
two non-metals to share 1 or more pairs of electrons
30
Metallic bonding involves attraction between
positive charged metal ions and delocalized negatively charged electrons.
31
What is an ionic compound
when millions of ions are held together by electrostatic forces between oppositely charged ions in the form of an ionic lattice
32
Properties of ionic compounds
``` Cannot conduct electricity in solid form as the ions are fixed and there are no free electrons When turned molten or dissolved in water ions are free and the electrons become delocalized allowing energy flow High MP and BP because a lot of energy required to break the ionic bonds in each ion Are hard (due to strong bonds) and brittle ```
33
Ionic compounds are structured in
alternating positive and negative ions in the form of a giant lattice structure
34
A covalent bond is the result of an
attraction between bonding pairs of electrons and the nuclei of an atom involved
35
When atoms covalently bond they become
molecules
36
Small covalent molecules are held by
strong covalent bonds
37
The forces between the covalent molecules are
weak intermolecular forces
38
Properties of small covalent molecules
Low BP and MP due to weak intermolecular forces Cannot conduct electricity due to no free electron Often gases and liquids at room temperature
39
Bigger molecules in small covalent molecules have
more intermolecular forces so as you go down the group 7 BP and MP gets bigger
40
What is an example of a double covalent bond
oxygen as they share 2 pairs of electrons (O2 = O2)
41
What is the display formula for covalent bond of Cl2
Cl - Cl
42
How many types of covalent bonds are there
3 | Single double and triple bonds
43
Ionic compound features
Volatility: Low State at room temp: Solid Solubility in water: High Electrical conductivity: Low (ions not free) Electrical conductivity in solution: High (ions are free)
44
Covalent bond features
Volatility: High State at room temp: Usually liquid or gas Solubility in water: Low Electrical conductivity: Low (no charge) Electrical conductivity in solution: Low (no charge)
45
What are giant covalent structures
Huge number of non-metal atoms and in regular repeating lattices
46
3 examples of giant covalent structures
Diamond, graphite and silicon dioxide
47
Properties of giant covalent bonds
One single molecule High BP and MP because loads of energy required to break every individual strong bond Don't conduct electricity even when molten (except graphite)
48
What are allotropes
Different forms or structures of the same element i.e Allotropes of carbon are diamond, fullerenes and graphite
49
Properties of graphite
Each carbon atom is bonded to 3 other carbon atoms They are hexagonal shape and within layers held by weak intramolecular forces. Layers are soft so slide over each other Graphite is soft Used as a pencil and is a lubricant Has free electrons so conducts heat and electricity
50
Properties of diamond
Very hard (used for cutting tools or to cut materials) Each carbon atom is bonded to 4 other carbon atoms Has high melting point Does not conduct electricity as no free electrons
51
A solid metal consist of
Giant structure of atoms in a regular pattern
52
How is a metal held in a regular structure
The metal atoms give up its electrons to share with other metal atoms. It forms a sea of delocalized electrons. The metal atoms become positively charged as they lost electrons and are electrostatically attracted to the negatively charged electrons which holds the metal together in a regular pattern
53
Why are alloys harder to break than pure metals
Since alloys consist of two or more different metallic elements the atoms are different sizes which disrupts the regular pattern and makes it harder to slide over the layers.
54
What are the layers in graphite called
graphene
55
Graphene can be shaped into tubes and spheres called
fullerenes
56
Use of fullerenes
Transport drugs Industrial catalyst Nanotubes

IGCSE Chemistry (16 decks)

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