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Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

Ionic bonding

A

Transferring electrons between metal and non metal atoms

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2
Q

Covalent bonding

A

Sharing electrons between two non metal atoms

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3
Q

Metallic bonding

A

Share free electrons between two metal atoms

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4
Q

Compounds

A

Atoms which have formed bonds with each other by chemical reactions

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5
Q

Electrostatic attraction

A

The attraction between oppositely charged atoms

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6
Q

Ionic bonds

A

Electrostatic attraction between oppositely charged ions

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7
Q

Intermolecular forces

A

Weaker bonds between multiple atoms of the same molecule

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8
Q

Simple molecular structure

A

Covalent bonds between the same element

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9
Q

Giant covalent structure

A

Regular lattice made by covalently bonded atoms

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10
Q

Regular repeating lattices

A

The same formation of atoms repeated in a lattice form

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11
Q

Malleability

A

Ability to be bent / hammered into shapes

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12
Q

Ductile

A

Ability to be drawn into wires

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13
Q

Sonorous

A

Makes a sound when hit

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14
Q

Ion

A

Atom or group of atoms with an electric charge due to transferring electrons

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15
Q

Cations

A

Positive ions

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16
Q

Ations

A

Negative ions

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17
Q

S+

A

Slighty positive ion

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18
Q

S-

A

Slightly negative ion

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19
Q

Delocalised

A

Not in a fixed position

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20
Q

Graphine

A

A single layer of graphite

21
Q

Allotropes

A

Different structural formations of the same element in the same physical state

22
Q

Macromolecules

A

Giant covalent strucure

23
Q

Alloy

A

A mixture containing one of more metal element

24
Q

Properties of ionic compounds

A
  • when solid, form white crystals and are not volatile
  • very high melting and boiling point
  • don’t conduct electricity unless moleten
  • solids are soluble in water
  • solids are insulators
25
Q

Zn2+

A

Zinc (positive ionic compound)

26
Q

Ag+

A

Silver - positive ionic compound

27
Q

H+

A

Hydrogen- positive ionic compound

28
Q

NH4+

A

Ammonium- positive ionic compound

29
Q

Fe2+

A

Iron- positive ionic compound

30
Q

OH-

A

Hydroxide- negative ionic compound

31
Q

HCO3-

A

Hydrogen carbonate - negative ionic compound

32
Q

What does ‘ide’ mean at the end of an ionic compound?

A

A simple compound made of two elements

33
Q

What does ‘ate’ mean on the end of an ionic compound?

A
  • another element often oxygen in involved
34
Q

What are properties of simple molecular structures?

A
  • easily change state
  • volatile
  • insulators
  • conduct when dissolved in water
35
Q

What does volatile mean?

A
  • evaporates easily (has a strong smell usually)
36
Q

What are the allotropes of carbon?

A
  • diamond, graphite, nano tubes, fullerines
37
Q

What are the properties of giant covalent structures? What are examples of giant covalent structures?

A
  • very high melting points
  • dont form molecules
  • form regular repeating lattices
  • all bonds are covalent (no intermolecular)
    Examples include diamond, graphite and silicon dioxide
38
Q

Properties of diamond

A

-very hard
- each carbon atom covalently bonded to 4 other carbon atoms
- doesn’t conduct
- giant covalent structure

39
Q

Properties of silicon dioxide

A
  • giant covalent structure
  • made up of silicon and oxygen
    Oxygen }2 silicon
    Silicon}4 oxygen
40
Q

In what type of structures are intermolecular forces ONLY used in?

A

Simple molecular

41
Q

What are the properties for graphite

A
  • composed of layers of graphine held together by weak intermolecular forces
  • high melting point
  • layers can slide off each other
42
Q

What are the properties of graphine?

A
  • hexagonal structure
  • a single layer of graphite
  • two delocalised electrons, so semi conductive
  • transparent
  • allotropes of carbon
43
Q

What are the properties of nano tubes?

A
  • stronger than steel (high tensile strength)
  • rolled graphine
  • good heat conductor
  • unique electrical properties
44
Q

What are the properties of Buckminster fullerene?

A
  • can’t conduct
  • 60 carbon atoms
  • used as a solid lubricant (like microscopic ball bearings)
  • each carbon atom bonded with 3 others (1=c-2)
  • hollow football shape
45
Q

What are the properties of metallic compounds?

A
  • high melting point as strong attraction between positive charged ions and sea of electrons
  • malleable
  • ductile
  • sonorous
  • conduct
  • strong and hard
  • shiny
46
Q

What is metallic bonding (process)

A
  • all metals form positive ions when creating a full outer shell s all in centre of periodic table
  • giant structures of positive ions create a regular lattice as they are packed tightly together
  • outer electrons become delocalised and separate toform sea of electrons
  • metal atoms become positively charged
  • sea of electrons becomes negatively charged so becomes attracted to metal atoms
  • sum of all electrons in the sea of electrons together make all the metal atoms have full shells
47
Q

Why are metals so strong?

A
  • metallic bonds don’t break as sea of electrons are free to move
48
Q

Why are metals pure metals more malleable ?

A
  • all metla atoms are same size and form layers
  • when hit the layers can slide over each other rather than breaking
49
Q

Why are alloys stronger than pure metals?

A
  • alloys are made up if two or more different metals
  • different metals have different size atoms
  • when alloys form layered structure, the different sized atoms make the layered structure impossible and therefore the layers cannot slide over each other

Chemistry (5 decks)

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