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IGCSE Chemistry > 3 Atoms, Elements and Compounds > Flashcards

3 Atoms, Elements and Compounds Flashcards

1
Q

Atomic number

A

number of protons inside the nucleus of an atom, determines the element

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2
Q

Nucleon Number

A

number of protons + neutrons in the nucleus

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3
Q

What determines an atom’s chemical property

A

Outer shell electron arrangment

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4
Q

Isotope

A
  • Atoms of the same element which have the same atomic number but different nucleon number
  • Same chemical properties because they have the same amount of electrons on the outer shell
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5
Q

Two types of isotopes

A
  • Radioactive

- Non-radioactive

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6
Q

One industrial and One medical use of radioactive isotopes

A
  • Cancer treatment
  • Tracers
  • Carbon dating
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7
Q

Element

A

substance consist of only one type of atom

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8
Q

Compound

A

substance made from two or more different type of atoms that are chemically bonded

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9
Q

Mixture

A

Consist of 2 or more different type of elements or compounds that are not chemically bonded

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10
Q

Properties of metals

A
  • Generally conductive
  • High melting point and boiling point
  • reacts to form positive ions
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11
Q

Alloys

A

Mixture of metals with other elements

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12
Q

Why are alloys harder than metals

A

+ions have different sizes and are in irregular arrangement

prevents the layers from sliding as easily

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13
Q

Cation

A

Positive ion

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14
Q

Anion

A

Negative ion

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15
Q

Describe lattice structure of ionic compound

A

regular arrangement of alternating positive

and negative ions

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16
Q

Covalent bonds

A

The sharing of a pair of electrons leading to the noble gas configuration

17
Q

Describe electron arrangement of N2

A

Triple bond

18
Q

Describe electron arrangement of C2H4

A

6 x Single bond

19
Q

Describe electron arrangement of CH3OH

A

4 x Single bond

20
Q

Describe electron arrangement of CO2

A

2 x Double bond

21
Q

Volatility of Simple Molecular covalent substances

A

High

22
Q

Volatility of Giant Covalent structures

A

Low

23
Q

Volatility of Ionic compounds

A

Low

24
Q

Solubility of Ionic compounds

A

Mostly soluble in water

Insoluble in other covalently bonded solvents

25
Q

Solubility of Covalent compounds

A

Insoluble in water

Soluble in other covalent type solvents

26
Q

Electrical conductivity of Ionic compounds

A
  • There are delocalised electrons to carry charge

- Only when molten or dissolved

27
Q

Electrical conductivity of covalent compounds

A

No delocalised electrons to carry charge

-except graphite

28
Q

Boiling point of Ionic compounds

A

High

  • Strong electrostatic attractions between oppositely ions
  • Require lots of energy to overcome
29
Q

Boiling point of giant molecular structures

A

High

  • All atoms are linked with strong covalent bonds
  • Require lots of energy to overcome
30
Q

Boiling point of simple molecular covalent structures

A

Low

  • Weak intermolecular forces between molecules
  • Low energy required to overcome
31
Q

Describe Diamond

A
  • Each carbon joined to 4 other carbons
  • Very hard due to the strong intermolecular forces between layers
  • High melting point
  • Does not conduct electricity
32
Q

Describe Graphite

A
  • Each carbon joined to 3 other carbons
  • Layers of hexagonal rings
  • Soft due to no covalent bonds between layers instead they have weak intermolecular forces
  • Conductive due to one delocalised electron from each carbon atom
33
Q

Describe Silicon (IV) dioxide

A
  • Each Silicon atom bonded to 4 Oxygen atoms
  • Each Oxygen atom bonded to 2 Silicon atoms
  • Empirical formula is SiO2
  • Too many atoms for Molecular formula
34
Q

Similar properties of Diamond and Silicon (IV) dioxide

A
  • Very hard
  • High melting points and boiling points
  • Insoluble in water
  • Does not conduct
35
Q

Metallic bonding

A

a lattice of positive ions in a ‘sea of electrons’

IGCSE Chemistry (3 decks)

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