Bonding Flashcards

1
Q

Metallic bonding

A

Electrostatic attraction between positive ions and delocalised electrons

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2
Q

Structure in metallic bonding

A

Giant metallic lattice

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3
Q

What attraction is broken when melting or boiling a substance with metallic bonding

A

Metallic bonds

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4
Q

Properties of metals

A

-Conductive as delocalised electrons are free to move and carry a current
-Malleable and ductile as layers of ions can slide past each other

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5
Q

Type of elements involved in ionic bonding

A

Mental and a non metal

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6
Q

Ionic bonding

A

Electrostatic attraction between oppositely charged ions

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7
Q

Structure in ionic bonding

A

Giant ionic bonds

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8
Q

Properties of compounds with ionic bonding

A

When molten they are conductive as ions are free to move and carry a current

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9
Q

Elements involved in covalent bonding

A

Two non metals

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10
Q

Covalent bonding

A

Started pair of electrons

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11
Q

2 types of Covalent structures

A

Marco and simple molecular

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12
Q

What is broken when melting or boiling a Macro molecular structures

A

Covalent bonds

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13
Q

What is broken when melting or boiling simple molecular elements

A

Intermolecular forces

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14
Q

Are macro molecular structures conductive

A

No except graphite

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15
Q

Are simple molecular compounds conductive

A

No as there is no electrons to carry The charge

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16
Q

Factors determining strength of metallic bonding

A

-size of an ion=smaller ion means stronger bonding
-charge of a metal ion=greater charge means stronger bonding
- number of delocalised electrons=more delocalised electrons means stronger bonding

17
Q

Factors determining strength of ionic bonding

A

-charge of ions=greater charge means stronger bonding
-size of ions =smaller ion stronger bonding

18
Q

Compare convalent bonds and intermolecular attractions

A

Convalent bonds are stronger, in simple molecular structures imf breaks at much lower temperatures than convalent bonds

19
Q

Coordinate bond

A

Both electrons in them shared pair have come from the same atom.On a diagram they are represented by an arrow

20
Q

Effect of lone pairs

A

Repel more than bonding pairs ,reducing the bond angle by 2.5

21
Q

Electronegativity

A

Ability of an atom to attract electron density in a covalent bond

22
Q

Factors affecting electro negativity

A

Shielding= less shielding means stronger electronegativity
Atomic radius=smaller radius means greater electronegativity
Charge=greater charge means greater electronegativity

23
Q

Trends in electronegativity

A

Across a period it increases , down a group it decreases

24
Q

Describe how induced dipole-dipole attractions occur

A

Random movement of electrons in one molecule results in uneven distribution of electrons,creating a temporary dipole in one molecule.this induces a dipole in a neighbouring molecules.dipoles attract

25
Q

Factors affecting the strength of induced dipole dipole

A

-Number of electrons as more electrons means stronger attraction
-shape of molecule as straight chain molecules have more surface contact than branched so stronger attraction

26
Q

Polar molecule

A

Not symmetrical, so individual dipoles don’t cancel out eg cf4

27
Q

Non polar

A

Symmetrical dipoles cancel out eg nh3 ch3F