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H Chemistry > Chemical Changes And Structure > Flashcards

Chemical Changes And Structure Flashcards

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1
Q

Metallic bonding

A

Li Be H
Na Mg Al
K Ca

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2
Q

Covalent network

A

B Si

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3
Q

Covalent molecule

A

C N O F
P S Cl

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4
Q

Monatomic

A

He Ne Ar

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5
Q

Properties of Metals

A

Good conductors of heat and electricity
Shiny
Malleable
Ductile
High melting points

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6
Q

Describe metals

A

Outer electrons can move easily from atom to atom. Delocalised electrons. Strong forces between the positive ions and delocalised electrons.

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7
Q

Properties of monatomic elements

A

Exist as individual atoms
Full outer energy levels
LDF’s are always present
Temporary dipole

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8
Q

Explain a temporary dipole

A

Continual movement of electrons in an atom which causes a temporary uneven distribution of charge at opposite sides of an atom, this means that one side is S+ and one side is slightly S-

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9
Q

What does having more electrons mean in terms of of LDF’s?

A

The LDFS are weak but with more electrons there is in the atom the bigger the LDFS

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10
Q

What is a covalent molecular bond?

A

It’s the mutual attraction of the nuclei for the shakers pair of electrons

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11
Q

What type of bonds are present and where in covalent molecular molecules?

A

Weak LDFS between molecules
Strong covalent bonds between atoms in the molecules

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12
Q

Properties of covalent network

A

Mon-metal, extremely high melting and boiling points
Silicon, carbon, boron

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13
Q

Explain diamonds properties

A

No delocalised electrons therefore it’s a non conductor of electricity, excellent conductor of heat. Hardest substance at room temp due to the closely packed atoms. 1 carbon bonds to 4 carbons

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14
Q

Explain the properties of carbon/graphite

A

Conducts electricity. Lead. 1 carbons bonds to 3 carbon cause the 4th carbon is delocalised therefore it conducts electricity

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15
Q

Explain the properties of silicon

A

Very high melting points, very hard, poor conductor of electricity. Semiconductor. Similar bonding to diamond. 1 carbon=4 carbon bonds

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16
Q

Explain the properties of boron

A

Similar bonding to carbon. 1carbon=3 carbon, 4th is delocalised. Stable covalent networks, very hard, high melting points

17
Q

How are covalent bonds made?

A

They are formed when non-metal atoms shaired a pair of electrons.

18
Q

How are the electrons shaired when in pure covalent?

A

They are shared equally and have the same electronegativity value

19
Q

What does it mean when it has a permanent dipole?

A

It’s polar covalent, which means it has a small difference in electronegativity

20
Q

What does it mean if it has ionic bonding?

A

Large difference in electronegativity. Also it’s the electrostatic force of attraction between positive and negative ions.

21
Q

If a molecule had permanent-dipole-permanent-dipole bonding what bonding does it have?

A

Polar

22
Q

How can you also tell if a molecule is polar or non-polar?

A

By looking at its structure

23
Q

Explain hydrogen bonding properties and how it’s formed

A

Highly electronegative elements, F,N,O. Highly polar and have very strong p-d-p-d interactions. They are the strongest van der waals forces

24
Q

how do you balance ion-electron equations?

A
  1. balance the number of elements
  2. add water to balance the oxygen
  3. add H to balance h atoms
  4. add electrons to balance the charge
25
Q

oxidising agents tend to be more….

A

positive

26
Q

reducing agents tend to become more…

A

negative

27
Q

acidified peroxide is…

A

an oxidising agent as it accepts electrons and is reduced itself

28
Q

acidified dichromate is…

A

an oxidising agent as it accepts electrons and reduces itself

29
Q

carbon monoxide is…

A

a reducing agent as it accepts electrons and is reduced itself

30
Q

Define the term first ionisation energy

A

The amount of energy to remove one mole of electrons from one mole of atoms in a gaseous state

31
Q

Electronegativity across a period

A

Increases due to increased nuclear charge

32
Q

Electronegativity down a group

A

Decreases due to the electrons being further away

33
Q

Ionisation down a group

A

Decreases due to an increased electron screening effect

34
Q

Ionisation energy across a period

A

Increases as you go across cause the increase in protons which means there is a stronger nuclear charge

H Chemistry (3 decks)

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