Prep For June Mocks Flashcards
(70 cards)
1
Q
Definition of an atom
A
The smallest particle of an element that can exist that is constructed of subatomic particles.
2
Q
Definition of an ion
A
An atom that has lost or gained an electron (has an overall charge)
3
Q
Definition of An isotope
A
The same element with a different number of neutrons, therefore changing the atomic number but not the charge
4
Q
What is meant by atomic number?
A
Number of protons in one atom of an element
5
Q
What is meant by mass number?
A
Number of nucleons in an atom (always a whole number)
6
Q
What are nucleons?
A
Protons and neutrons
7
Q
What is the mass of an electron
A
1/2000
8
Q
What subatomic particles are found in the nucleus?
A
Protons and neutrons
9
Q
Definition of orbitals
A
A region of space that can hold up to 2 electrons with opposite spins
10
Q
How many orbitals are there in subshell s?
A
1
11
Q
How many orbitals are there in subshell p?
A
3 ( max no of electrons:6)
12
Q
How many orbitals in subshell d?
A
5 ( max no of electrons:10)
13
Q
How many orbitals in subshell f?
A
7 ( max no of electrons:14)
14
Q
Ammonia
A
NH3
15
Q
Ammonium
A
NH4
16
Q
Methane
A
CH4
17
Q
Hydrochloric acid
A
HCl
18
Q
Sulphuric acid
A
H2SO4
19
Q
Nitric acid
A
HNO3
20
Q
Hydroxide
A
OH-
21
Q
Carbonate
A
CO3 2-
22
Q
Sulphate
A
SO4 2-
23
Q
Nitrate
A
NO3-
24
Q
Amount of substance =
A
Mass of substance (g) / molar mass (gmol -1)
25
Moles =
Mass / Mr
26
Amount of substance (mol)=
Number of particles/Avogadros number
27
Stoichiometry definition
The relative number of moles of each substance that react
28
Stoichiometry steps
1) turn the mass given into moles
2) look at the relationship between the moles of the element in the equation
3) work out the number of moles of the substance you’re asked about
4) concert that into mass
29
Molecular formula?
Shows the number of atoms of each element in one molecule of the substance
30
Empirical formula?
Simplest whole number ration of atoms in element
Divide by mass
Divide by Ar
Divide by smallest
31
What is a hydrated salt?
When a salt has water of crystallisation
32
What is an anhydrous salt?
A salt without water of crystallisation
33
%mass =
(Mass of element in the compound /total mass of compound )x100
34
Definition of an acid?
A compound that releases protons in aqueous solutions (proton doner)
35
Definition of a base?
The h+ released from an acid accepts a pair of electrons from a base to form a new compound or ion (proton acceptor)
36
Definition of an alkali
Alkalis release OH- ions in aqueous solution
37
Definition of a salt
A compound formed when the H+ ions from an acid is replaced by a metal ion or an ammonium ion
38
What is a strong acid?
An acid that is completely ionised in aqueous solution
39
What is a weak acid?
An acid that is only partially ionised in aqueous solution
40
What are the steps for creating an ionic equation?
1) write down normal equation
2) write out again with all the ions separated
3) if an ion appears on both sides it cancels out
41
Concentration(moldm-3)=
Number of moles of solute/volume of solution(dm3)
42
How do you get from cm3 to dm3?
Divide by 1000
43
How do you get from dm3 to cm3?
X 1000
44
Concentration after dilution=
Moles/new volume
45
Volume of gas=
Moles x 24
46
What is the ideal gas equation?
P=nRT/v
47
What do the letters stand for in the ideal gas equation?
P=nRT/v
```
P= pressure in pa
V= volume in m3
N= number of moles
R= absolute temperature in k
T= gas constant
```
48
How do you get pressure in pa?
Pa =kpa x 1000
49
How do you get m3 from dm3?
M3= dm3 / 1000
50
How do you work out absolute temperature in k?
K= temperature (c) +273
51
What is the definition for the first ionisation energy?
The energy needed to remove one electron from each atom is a mole of gaseous atoms of an element
52
What is the equation for the first ionisation energy?
X(g)—> X+(g)+e-
53
What are the factors affecting ionisation energies?
1) nuclear charge
2) atomic radius
3) shielding
54
How does nuclear charge affect ionisation energy?
The higher the nuclear charge the stronger the electrons attraction to the nucleus so the higher the IE
55
How does atomic radius affect the ionisation energy?
The greater the atomic radius the weaker the attraction between the electrons and nucleus so the lower the IE
56
How does shielding affect the IE?
The greater the number of shells the greater the shielding so the lower the IE because the electrons are easier to remove
57
What shell is the electron from?
Outer shell
58
Trends in the successive ionisation energies?
1) there is always an increase in the IE with every successive electron removed
2) there is always a large increase in the IE when a shell is lost and the electron being removed is in a different shell
59
Why is there always an increase in IE with every electron removed?
Because there are less electrons so less repulsion which means the atomic radius is slightly smaller therefore the electrons are more attracted to the nucleus because they are closer. This means that the successive electrons being removed require more energy
60
Why is there a large increase in IE when a shell is lost and the electron is being removed from s different shell
Because there are less shells the atomic radius is smaller meaning the electrons are more attracted to the nucleus and require more energy to be removed
61
Why does the first ionisation energy increase across a period?
Because the number of shells stays the same but the nuclear charge increases do the electron is more attracted to the nucleus.
62
Why does the ionisation energy decrease between group 2 and group 3 elements?
Because the highest energy electron is in the p subshell for group 3 but in the s subshell for the group 2 element and because the p subshell is at slightly higher energy than the s subshell it is slightly easier to remove an electron from the group 3 element
63
Why does the ionisation energy between the group 5 and 6 element decrease?
Because the highest energy electron is a paired p electron for the group 6 element but an unpaired p electron for the group 5 element. And due to repulsion between paired electrons which raises their energy it is slightly easier to remove the paired outer electron from group 6
64
What is ionic bonding
The electrostatic attraction between positive and negative ions
65
In ionic substances what is the structure
Giant ionic lattice
66
Ionic compounds boiling points are?
High melting and boiling points because a lot of energy is needed to overcome the strong attractive forces between oppositely charged ions
67
Do ionic compounds conduct electricity?
Yes when they are molten or dissolved in aqueous solution however they cannot conduct when solid because there are no mobile electrons or ions.
68
Are ionic compounds soluble
Yes because they form ion-dipole bonds with water
69
What is a covalent bond
A covalent bond is the attraction of a shared pair of electrons for the nuclei of the bonded atoms
70
What group is an exception to the “8 electron” guideline?
Group 3
