Bonding Flashcards

1
Q

What is ionic bonding and give an example

A

Strong electrostatic forces between oppositely charged ions in a lattice
E.g NaCl (salt)

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2
Q

Describe and explain why ionic bonding has its properties?

A

High m.p. and b.p. —> requires lots of energy to break electrostatic forces
Conducts electricity —> when in solution ions are free to carry charge

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3
Q

What is simple molecular covalent bonding?
Give some of its properties

A

Strong covalent bonds between atoms but weak Van der Waals
Cannot conduct electricity (electrons aren’t free to move)
Has a low m.p. and b.p. (weak VdW)

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4
Q

Describe macromolecular bonding and give some of its properties

A

Lattice of many atoms held together by covalent bonds
High m.p. and b.p.
Doesn’t conduct electricity

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5
Q

Compare and contrast the structure of diamond and graphite

A

Both have a macromolecular covalent structure
Each C in diamond is bonded to 4 others
In graphite each C is only bonded to 3

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6
Q

Describe metallic bonding

A

Lattice of +ve metal ions strongly attracted to a sea of delocalised electrons

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7
Q

Explain the trends and properties of metallic bonding

A

High m.p. and b.p. —> strong attraction betwenn +ve ions and -ve electrons
Conduct electricity —> delocalised electrons can carry charge
Strength of bond increases across the period —> more delocalised electrons which means a stronger force between them

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8
Q

Define electronegativity (EN)

A

Ability of an atom to attract the pair of electrons in a covalent bond

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9
Q

What affects EN?

A

Nuclear charge
Atomic radius
Electron shielding

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10
Q

What’s the difference between a non-polar and polar bond?

A

Non-polar = both bonding atoms have the same EN
Polar = bonding atoms have different EN

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11
Q

Describe Van der Waals force of interaction

A

Random movement of electrons creates temporary dipoles
Induces dipole in neighbouring molecule
Temporary induced dipole-dipole (VdW)

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12
Q

Describe a permanent dipole-dipole attraction

A

Molecules with polar bonds have permanent dipoles
Attraction between those dipoles and neighbouring molecules

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13
Q

What is a dative/co-ordinate covalent bond?

A

When an electro deficient atom accepts a lone pair of electrons from another atom

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14
Q

Name the shape, bond angle and how many bonded and lone pairs there are

A

Linear = 180 —> 2b, 0l
Trigonal Planar = 120 —> 3b, 0l
Tetrahedral = 109.5 —> 4b, 0l
Trigonal bypyramid = 90 and 120 —> 5b, 0l
Octahedral = 90 —> 6b, 0l

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