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Chemistry revision Flashcards

1
Q

What are of subshells ?

A

S, P and D

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2
Q

What order are the subshells filled and how many electrons do they hold ?

A

1s2 , 2s2, 2p6, 3s2, 3p6, 4s2,3d10

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3
Q

How are the subshells emptied ?

A

4s before 3d

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4
Q

what are orbitals ?

A

It is a region of space where an electron is likely to be found

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5
Q

How are arrows placed in orbitals ?

A
  • with the same energy must be filled singly before electrons are paired
  • the spins of the 2 electrons are opposite to each other
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6
Q

How do you name a compound with a metal and a non metal ?

A

Metal followed by non metal name ending in ide, e.g. oxide

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7
Q

What are the 3 types of bonding and where do they occur ?

A

Ionic - metal and non metal
covalent- non metal
metallic - metal

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8
Q

what are the physical properties of ionic substances ?

A
  • high melting and boiling point
  • don’t conduct electricity when solid but do when molten or dissolved
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9
Q

Why do ionic compounds have their substances ?

A

There is a strong electrostatic force of attraction between postive and negative ions, giant ionic structure is a lattice of many ions held together by electrostatic attraction

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10
Q

What factors affect the strength of ionic bonds ?

A
  • the strength of electrostatic attraction increases with increasing inoic charge and strength of electrostatic attraction decreases with increazing size of ionic radius
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11
Q

what is the trend in Ionic radius down a group ?

A

Ionic radius increases down a group as you get more shells

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12
Q

How does Ionic radius change across a period for groups 1,2,35,6 and 7 ?

A

It decreases across a period as you have a stronger postive charge in the nucleus.

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13
Q

What happens when a metal reacts in Ionic compounds ?

A

They lose electrons to become postive ions.

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14
Q

What happens when a metal reacts in Ionic compounds ?

A

They gain electrons to become negative ions

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15
Q

How many electrons are in the outer shell of an element ?

A

The group number

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16
Q

What happens in covalent bonding ?

A

The atoms share a pair of electrons

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17
Q

What are the proporties of covalent molecules ?

A

Simple covalent molecules have low melting and boiling points. They do not conduct electricity

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18
Q

What is a dative bond and some examples ?

A

It is a covalent bond in which the pair of electrons being shared is being donated by 1 atom

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19
Q

What happens as the number of electrons in a bond increase ?

A

As the number of electrons between two atoms increases, the bond strength increases

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20
Q

What shape do carbon molecules form ?

A

Carbon has 4 outer shells electrons so can form uo to 4 single bonds/bonding electron pairs and will form tetrahedral shapes

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21
Q

What angle is found in a tethedral shape ?

A

109.5 degrees

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22
Q

What is the structure of a metal ?

A

A lattice of postive metal Ions surrounded by delocalised electrons . Metallic bonding is the electrostatic attraction between the nuclei of the postive metal ions and the delocalised electrons

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23
Q

What is a giant metallic structure ?

A

It is a lattice of many atoms held together in regular layers by metallic bonding

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24
Q

how do the chemical and physical properties of metals, such as melting and boiling point,

malleability, ductility and electrical conductivity, are affected by their bonding and structure?

A

● High melting points dues to strong electrostatic forces between ions. Malleable and ductile as

regular ion layers slide over each other. Delocalised electrons are free to move throughout

structure so good conductors

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25
What holds simple covalent molecules together ?
Weak intermolecular forces
26
What are the 3 main types of intermolecular forces and their relative strengths ?
London = Weakest Permanent Dipole Dipole forces= middle Hydrogen Bonding = Strongest
27
When do london forces occur ?
In all atoms and Molecules.
28
How did London Forces occur ?
It is caused by having more electrons distributed on one side of the molecule that the other create small dipoles . This includes dipoles in nearby molecules
29
When does Dipole Dipole forces occcur and what happens ?
This occurs when an electronegative element is bonded to a non electronegative element . The electronegative element pulls electrons towards it to get a negative dipole and other elements get a postive dipole. They attract Nearby oppositely charged dipoles
30
When does Hydrogen bonding occur and what happens ?
It occurs when hydrogen is bonded to Flurione, Nitrogen or Oxygen. This is becuase hydrogen is not electronegative whilist Fluorine, nitrogen and oxygen are. Hydrogen gets a postive dipole . It is attracted to nearby lone pair of electrons . Flurione , Nitrogen and oxygen get a negative dipole as pull bonding electrons towards them
31
what are van der woels ?
London Forces
32
What is the formula of ions containing more than 1 element ?
hydroxide (OH-), carbonate (CO32-), sulfate (SO42-), nitrate (NO3-), ammonium (NH4+)
33
What are the state symbols (s), ( l) , ( g)
S - solid L - Liquid G - Gaseous solution
34
What is the relative atomicl mass of an element ?
The mean mass of isotopes of an element compared to 1/12 th of the mass of a carbon 12 atom
35
What is a mole ?
1 mole of any substance contains the same number of particles as there are atoms in 12 grams of carbon
36
How many particles in a mole ?
6.02 x 10 23
37
How do you convert moles into number of particles using the Avogrado constant ?
Moles x Avogrados Number
38
What is Concentration ?
It is the number of moles of a substance dissolved in water to prooduce a volume of 1dm cubed of a solution and has units of mol dm cubed
39
how do you calculate the number of moles ?
Moles = Mass / MR
40
How do you calculate concentration of a solution , the number of moles and volume of the solution ?
Concentration = Moles / Volume
40
How do you calculate the percentage yield of a product from an actual yield
Actual mass/ Experimental mass x 100
41
What is the order on the periodic table ?
Elements are arranged in order of increasing atomic number
42
Where are metals and non metals located on the periodic table ?
Metals = Left Non Metals = Right top corner
42
what does the period number tell you ?
Elements in the same period have the same number of occupied shells in their atoms
43
What does a group number tell you ?
Elements in a Group have the same number off electrons in the outermost shell of their atoms
44
Why are elements in each block of the periodic table ?
Highest subshell occupied by electrons will determine which block of the periodic table an element is found in
45
what is first ionisation energy ?
It is the energy required to remove 1 mole of electrons from 1 mole of atoms in their gaseous state
46
What is the equation for 1st Ionisation ?
X (g) a X + (g) + e -
47
what is the trend in Ionisation energy down a group in the periodic table and why ?
It decreases down a group as the electron being removed is further from the positive nucleus so less attracted to the nucleus, there is more shielding of the positive charge
48
what is the general trend in Ionisation energy across a Period ?
It increases across a period but that there are anomalies at group 3 and group 6 . This is because across a period there are more protons so a stronger nuclear charge but the same amount of shielding.
49
what is first electron affinity ?
It is the energy released when 1 mole of gaseous atoms gain 1 mole of electrons
50
Why does atomic radius changes across a period and down a group and why ?
It increases down a group as more shells making it bigger. It decreases across the period as more protons in the nucleus but same number of shells. Bigger attraction between the outer shell and the nucleus
51
What is electronegativity ?
It is a measure of the tendency of an atom to attract a bonding pair of electrons in a covalent bond
52
What happens to trends in electronegativity across a period and down a group ?
It decreases down a group as more shells making it bigger so less attraction between nucleus and electrons It increases across the period as more protons in the nucleus but same number of shells . Bigger attraction between the electrons and the nucleus
53
What is oxidation ?
Oxidation is the loss of electrons or the gain of oxygen
54
What is Reduction ?
Reduction is the gain of electrons or loss of oxygen
54
what are the rules to determine oxidation number ?
Group 1 metals always +1 Group 2 metals always +2 Oxygen is usually -2 except in peroxides and F2O Hydrogen is usually +1 except in metal hydrides where it is - 1 Fluorine always -1 Chlorine usually -1 except in compounds With Oxygen or Fluorine
55
What elements can have variable oxidation states ?
Transition metals can have ions with different oxidation numbers
56
What are the trend in the periodic table ? Why do we see these trends ?
As you go down a group you get more shells , electrons are less attracted to nucleus As you go across a period you get more protons but have the same number of shells , electrons are more attracted to nucleus
57

Btec Applied science (20 decks)

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