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Chemistry > Bonding > Flashcards

Bonding Flashcards

(49 cards)

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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

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A

A single layer of graphite

21
Q

Allotropes

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A

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

22
Q

Macromolecules

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A

Giant covalent strucure

23
Q

Alloy

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A

A mixture containing one of more metal element

24
Q

Properties of ionic compounds

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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
Zn2+
Zinc (positive ionic compound)
26
Ag+
Silver - positive ionic compound
27
H+
Hydrogen- positive ionic compound
28
NH4+
Ammonium- positive ionic compound
29
Fe2+
Iron- positive ionic compound
30
OH-
Hydroxide- negative ionic compound
31
HCO3-
Hydrogen carbonate - negative ionic compound
32
What does ‘ide’ mean at the end of an ionic compound?
A simple compound made of two elements
33
What does ‘ate’ mean on the end of an ionic compound?
- another element often oxygen in involved
34
What are properties of simple molecular structures?
- easily change state - volatile - insulators - conduct when dissolved in water
35
What does volatile mean?
- evaporates easily (has a strong smell usually)
36
What are the allotropes of carbon?
- diamond, graphite, nano tubes, fullerines
37
What are the properties of giant covalent structures? What are examples of giant covalent structures?
- 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
Properties of diamond
-very hard - each carbon atom covalently bonded to 4 other carbon atoms - doesn’t conduct - giant covalent structure
39
Properties of silicon dioxide
- giant covalent structure - made up of silicon and oxygen Oxygen }2 silicon Silicon}4 oxygen
40
In what type of structures are intermolecular forces ONLY used in?
Simple molecular
41
What are the properties for graphite
- composed of layers of graphine held together by weak intermolecular forces - high melting point - layers can slide off each other
42
What are the properties of graphine?
- hexagonal structure - a single layer of graphite - two delocalised electrons, so semi conductive - transparent - allotropes of carbon
43
What are the properties of nano tubes?
- stronger than steel (high tensile strength) - rolled graphine - good heat conductor - unique electrical properties
44
What are the properties of Buckminster fullerene?
- 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
What are the properties of metallic compounds?
- high melting point as strong attraction between positive charged ions and sea of electrons - malleable - ductile - sonorous - conduct - strong and hard - shiny
46
What is metallic bonding (process)
- 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
Why are metals so strong?
- metallic bonds don’t break as sea of electrons are free to move
48
Why are metals pure metals more malleable ?
- all metla atoms are same size and form layers - when hit the layers can slide over each other rather than breaking
49
Why are alloys stronger than pure metals?
- 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

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