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Materials > Bonding > Flashcards

Bonding Flashcards

1
Q

Name the three primary bonding

A

Ionic
Covalent
metallic

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2
Q

Name the three secondary bonding types

A

Van der waals
Hydrogen bonding
Dipole dipole

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3
Q

What is valency

A

The measure of the number of electrons either lost shared and gained during Bonding

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4
Q

State the octate rule

A

An atom which has 8 electrons in its outer shell won’t bond
Platinum
Gold

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5
Q

What is ionic bonding?

A

Transfer of electrons between a metal and a non metal to acquire a stable config of a noble gas
Strong electrostatic attraction due to oppositely charged ions.
Repulsive component due to overlapping electron cloud.
High mp, high solubility.
Can conduct
Forms when an atom that can easily lose electrons to an atom that easily gains electrons

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6
Q

What is covalent bonding?

A

Sharing of electrons between two non metals to form an inert has config
No free electrons
Electrons localised and form directional bonds
Low mp
Soft
Uses secondary bonding

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7
Q

What is a sigma bond?

A

Head on overlapping between atomic orbitals

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8
Q

What is a Pi bond?

A

Covalent bonds where two loves of one involved atomic orbital overlap two lives of the other involved atomic orbital

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9
Q

What is electron pair repulsion theory?

A

Only outer electrons involved in bonding.

Electron pairs repel other pairs and move away which dictates the shape and the angle

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10
Q

What is metallic bonding?

A

Bonding using delocalised electrons which create strong bonds

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11
Q

Why is Mg stronger than Na?

A

Mg has more free electrons therefore a higher electron density and twice the charge.
Can form more attractions between the free electrons.
It has one more electron than Na so has greater charge
Smaller radius so electrons closer to the nucleus.
Higher melting point

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12
Q

Why does atomic radius decrease across a group?

A

More positive charge, so the atom is held more tightly as shells are pulled together.

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13
Q

Why does atomic radius increase down a group?

A

More shielding
More shells
Held less tightly

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14
Q

Why are transition elements roughly the same size?

A

Due to nuclear charge, and the distance between the 4s orbital and the repulsion between the 3d and the 4s electrons are in balance

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15
Q

What is electronegativity?

A

Relative attraction an atom has for the shared pair of electrons in a covalent bond within a molecule

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16
Q

Why does electronegativity decrease down a group?

A

Nucleus has smaller attraction for bonding due to being further away .
More shells and shielding

17
Q

Why does the electronegativity increase across a group?

A

Charge increases, reduction in radius, nucleus has greater attraction

18
Q

What is a polar molecule

A

Where there is an uneven distribution of charge

19
Q

What is a non polar bond

A

Same density, uncharged etc

20
Q

What is a dipole?

A

Due to unequal sharing of electrons, there is positive charge separated by a short distance from a centre of negative charge.

21
Q

What is a dipole moment?

A

Measures the tendancy of the molecule to turn when placed in an electric field.

22
Q

What type of molecule will have a 0 dipole moment

A

Non polar molecule, linear

23
Q

How do you test for a dipole?

A

Place a charged rod into a liquid.

If the liquid attracts then there is a dipole

24
Q

What is an intramolecular force?

A

They are forces of attraction

25
Q

What is an intermolecular force?

A

Force which Determines the state of a compound

26
Q

What is a dipole dipole attraction?

A

When two molecules pull closer together due to charge

27
Q

What is a van der waal?

A

When more electrons lie to one side, this creates a temporary instantaneous electric dipole.
This electric dipole creates an induced dipole in a neighbouring molecule.
Weakest type of force
Large molecules can be strong

28
Q

What is hydrogen bonding?

A

Bonding due to the difference in electronegativity between hydrogen in oxygen, nitrogen and Florine
Highly polarised, permanent dipole set up

29
Q

What type of bond will form with similar electronegativity

A

Covalent

Close to non polar

30
Q

What type of bond will form with a big difference in electronegativity

A

Ionic

Polar bond

Materials (11 decks)

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