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Chemistry > Atoms, Bonding & Structures F4 > Flashcards

Atoms, Bonding & Structures F4 Flashcards

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1
Q

Plum Pudding Model

A
  • Thomson

- Electrons are dotted through a positively charged sphere.

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2
Q

Modern Model of Atom

A
  • Rutherford

- Positive nucleus is orbited by electrons.

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3
Q

Who discovered neutron?

A
  • Chadwick

- Neutral

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4
Q

Atom

A

Simplest part of element that can exist and take part in chemical reactions.

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5
Q

Element

A

Pure substance which contains only one type of atom.

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6
Q

Compound

A

Pure substance which contains two or more elements chemically combined.

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7
Q

Mixture

A

Substance which is not chemically combined and can be easily separated.

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8
Q

What does the number is electrons in outermost shell indicate?

A

Group number.

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9
Q

Isotopes

A

Atoms with the same atomic number but different mass number.

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10
Q

Ions

A

Charged particles formed when an atom either loses or gains electrons.

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11
Q

What are CATIONS?

A

Positively charged ions.

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12
Q

What are ANIONS?

A

Negatively charged ions.

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13
Q

What is the radius of an atom?

A

0.1nm

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14
Q

1nm =

A

= 1 x 10-9m

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15
Q

Radius of nucleus

A

1/10,000

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16
Q

Alloy

A

Mixture of 2 or more elements, at least one of which is a metal.

Has metallic properties.

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17
Q

What is steel an alloy of?

A

Iron and Carbon.

18
Q

Bonding

A

How atoms / ions are held together

19
Q

Structure

A

How atoms / ions are arranged

20
Q

Metallic Structure

A 
METALLIC BONDING
Attraction between positive ions and delocalised electrons. 
- High melting and boiling points 
   (attraction between positive ions and delocalised electrons) 
- Good conductors 
   (delocalised electrons)
- Malleable (can be hammered into shape)
- Ductile (can be drawn into wire)
21
Q

Giant Ionic Lattice Structure

A

IONIC BONDING
Ionic attraction between oppositely charged ions.
- High melting and boiling points
(substantial amount to break bonds of oppositely charged particles)
- Good conductors
- Soluble
SODIUM CHLORIDE

22
Q

Molecular Covalent Structure

A 
COVALENT BONDING
(O2, H2O, NH3)
- Strong covalente bonds
- Low melting and boiling points
   (weak Van de Waals’ forces between molecules)
- Don’t conduct
   (molecular covalent have neutral particles)
- Insoluble
23
Q

Giant Covalent Structure

A 
COVALENT BONDING
- 3D structure joined by covalent bonds 
- Large continuous networks of covalently bonded atoms 
• Diamond
• Graphene
• Graphite
- All made of Carbon
24
Q

Allotropes

A

Different forms of the same element in the same state.

25
Q

Diamond

A
  • Each carbon atom covalently bonded to 4 others
  • Very hard due to strong covalent bonds
  • Very high melting and boiling points because of covalent bonds
  • Doesn’t conduct
    (no free ions / delocalised electrons)
26
Q

Graphite

A
  • Most common form of Carbon
  • Layers of Carbon atoms arranged in hexagons
  • Weak Van de Waals’ forces between layers
  • One electron per carbon atom is unbonded
    (delocalised electrons)
  • Soft because layers can slide past each other due to weak Van de Waals’ forces
  • Good conductors
    (unbonded electron)
27
Q

Graphene

A
  • One atom thick layer
  • Strong Covalent bond between each atom
  • Very high melting and boiling points
    (substantial energy)
  • Very strong due to strong covalent bonds
  • Good conductor as one electron per carbon atom is unbonded
    (delocalised electrons)
28
Q

Ionic Bonding

A
  • Metal & Non-Metals
  • Electrons transfer from metal to non-metal
  • Opposite charged ions attract to form large regular structures.
29
Q

Covalent Bonding

A
  • 2 or more non-metal atoms, sharing electron pairs
  • Uncharged particles due to no ions
  • Shared electrons attract nucleus of atom
30
Q

Molecule

A

Two / more atoms covalently bonded together.

31
Q

Diatomic

A

Two atoms covalently bonded in molecule.

32
Q

Lone pair of electrons

A

2 / more unbonded electrons in molecules.

33
Q

Metallic Bonding

A
  • Attraction between positive metal ions in regular lattice and delocalised electrons
34
Q

Delocalised electrons

A

Electrons that are free to move throughout the whole structure.

35
Q

Covalent Bonds

A

One pair - SINGLE covalent
Two pairs - DOUBLE covalent
Three pairs - TRIPLE covalent

36
Q

What is used in ALLOYS?

A

Gold
Silver
Copper
Zinc

37
Q

How to find % of gold?

A

% = no. of carats/24 x 100

38
Q

How to find amount of carats (K)?

A

K = % x 24 / 100

39
Q

Nanoparticles

A

Structure that is 1-100nm in size and contain a few hundred atoms.

40
Q

Surface Area to Volume Ratio

A

As the size of a cube increases, the surface area to volume ratio decreases.

41
Q

Benefits of Nanoparticles

A
  • Better skin coverage to sun cream
  • More effective protection
  • Clear and colourless
  • Does not degrade on exposure to sun
42
Q

Major Risks of Nanoparticles

A
  • Harmful effects on humans & environment
  • Potential cell damage in body
  • More reactive / more toxic than bulk material

Chemistry (11 decks)

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