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Science 2024 > C1 > Flashcards

C1 Flashcards

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1
Q

For each electron shell 1-5 what is the maximum number of electrons

A

1-2
2-8
3-18
4-32
5-50

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2
Q

What is an orbital

A

Regions where there Is 95 percent probability of locating an electron
An orbital can hold up to two electrons
There are s,p,d,f orbitals

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3
Q

What is electron figuration

A

The distribution of electrons in an atom/molecule

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4
Q

Ionic bonding

A

Electrostatic attraction between two oppositely charged ions

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5
Q

What group are nobles gases

A

0

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6
Q

What is the main feature about noble gases and how does this make it different to other elements in other groups

A

Have full outer shells which means they do not react easily and do not react at all compared to other elements that do not have outer shells which allows them to react to gain stable electronic configurations

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7
Q

What is a giant ionic lattice

A

Regular arrangement of positive and negative ions

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8
Q

When does the electrostatic force become stronger in a ionic bond

A

When the ionic charge is higher

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9
Q

When does the electrostatic force become weaker in an ionic bond

A

When the ionic radii are bigger as when the ionic radius is bigger the ionic charge is spread over a large surface area

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10
Q

What is covalent bonding

A

Occurs between two non metals it forms when an electron is shared between atoms

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11
Q

What is a dative covalent bond

A

When covalent molecules sharing electrons that come from one atom. For example oxygen and oxygen

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12
Q

What is a triple covalent bond

A

When three pairs of electrons are shared

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13
Q

What bond is stronger out of single,double or triple covalent bond and why

A

Single bonds have a greater length than double and double has a greater length than triple. The shorter the length of the bond the stronger it is

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14
Q

What is a lone pair

A

A non binding electron/ electrons that haven’t been joined to a different shell

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15
Q

Organic compound

A

Compound that contains one or more carbons

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16
Q

What structure does methane have and why

A

Tetrahederal structure as the bonds are separated because the negative electrons repel from one another
It is a 3d shape

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17
Q

Metal held by

A

Structures of atoms are held by metallic bonding

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18
Q

Delocalised electron

A

Electrons that are free to move and are present in metal but no covalent bonds or single atoms

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19
Q

What does delocalised electrons allow in metallic bonding

A

Gives the metal nuclei a positive charge which is attracted to the negative charge on the delocalised electrons which creates a strong force of attraction

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20
Q

Is metallic bonding stronger than covalent or ionic

A

No

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21
Q

How can you determine what type of bond will form between two atoms

A

Electrongetavity as it has the tendency to attract a bonding pair of electrons

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22
Q

If atoms have similar electronegativities what do they form

A

Covalent bond

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23
Q

Non-polar meaning

A

A molecule where the electrons are distributed evenly throughout the molecule which means in a covalent bond when the electrons have been shared between them to make the atom stable and must have the same electronegativity

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24
Q

Polar covalent meaning

A

Uneven electron distribution as shared electrons are more attracted to one nucleus more than the other. The atom with higher electronegativity will attract more electrons which gives the atom a slight negative charge and the other will have a slight positive charge

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25
Q

Intermolecular force

A

Th attraction/repulsion between neighbouring forces

26
Q

One type of intermolecular force

A

London dispersion forces/temporary dipole-induced dipole forces

27
Q

What is a London dispersion force

A

Weak forces between non-polar covalent molecules

28
Q

What is a dipole

A

Separation of charges within a covalent molecule

29
Q

What causes a temporary diple

A

When the electrons distribution becomes non-symmetrical

30
Q

Due to the electrons having a temporary dipole what can happen to the electrons in a nearby molecule

A

Repels the electrons which induces(causes) a dipole in that molecule

31
Q

Once there is an induced dipole what happens between it and the temporary dipole

A

Attract each other and pull the molecules together but forces are temporary as the electrons are constantly moving so electron density in the molecule is changing
Larger molecules have more electrons which means the force is bigger

32
Q

When is there london dispersion forces

A

Forces that exist between noble gases and non polar molecules

33
Q

What r the main 4 points of london dispersion forces

A

If there are more electrons there is more movement which leads to bigger dipoles and a stronger attraction

34
Q

What are dipole-dipole forces and are they stronger than London dispersion forces

A

Permanent forces between polar molecules
Yes they are stronger but weaker than covalent bonds

35
Q

What molecules does there have to be to be a dipole-dipole force

A

Hydrogen chloride and iodine monichloride
Plus the chlorine atom is slightly negative and the hydrogen and iodine atoms are slightly positive

36
Q

What is the strongest intermolecular force

A

Hydrogen bond

37
Q

When will hydrogen bonds form

A

When compounds have hydrogen bonded to fluorine, oxygen or nitrogen as there is a large difference in electronegativity between hydrogen and these atoms

38
Q

What does this large difference lead to

A

Polar bonds are formed and so the molecules have permanent dipoles and there will be an attraction between the positive side and lone pair side

39
Q

Calculation for mass

A

Mass=molar mass×number of moles

40
Q

Relative atomic mass

A

Tells you how much mass there is in one mole of the element

41
Q

Relative formula mass

A

Sum of all the relative atomic masses of all atoms in formula

42
Q

Standard solutions

A

Using solution of a known concentration as these have been prepared to ensure specific concentration is needed

43
Q

Concentration formula

A

Number of moles of solute divided by volume of solvent

44
Q

Titration

A

A method used to calculate concentration of a solution

45
Q

Solution

A

A liquid mixture where a solute is dissolved in a solvent

46
Q

Solute

A

Substance dissolved in a solvent to form a solution

47
Q

Solvent

A

A liquid that dissolveelsbanother substance

48
Q

What does s,l,g mean next to an equation

A

Solid,liquid and gas

49
Q

What does aq mean next to an equation

A

Solution

50
Q

Stochiometry

A

Using relationships between reactants and products in a chemical reaction to work out how much product will be produces from given amounts of reactants

51
Q

Theoretical mass

A

The expected amount of product from a reaction calculated from balanced equation

52
Q

Why do people use the percentage yield equation

A

To know how efficient their reaction process is

53
Q

Percentage yield equation

A

Actual mass /theoretical mass ×100

54
Q

Ionisation energy

A

Energy requited to remove one mole of electrons from atoms in their gaseous state

55
Q

How does an atom turn into an ion

A

Gains electrons

56
Q

What is a transition metal

A

Metals rhat form more than one stable ion with an incomplete d sub shell
They a re a subset of d block elements
D block elements are elements where the last two electrons to fill the atom is placed into a d orbital
Incomplete d sub shell explains some fo the key properties or transition metals

57
Q

How does gold conduct electricity

A

Metallic structure
Delocalised electrons
Electronsnare free go move
Electrons carry current

58
Q

Whay foes it mean if the proton does not have a whole number

A

Different isotopes
Isotopes have different abduncies
Relative mass is weighed averagely

59
Q

Redox reaction

A

Oxidation and reduction
Explain what what are

60
Q

How do delocalised electrons affect thermal or conduct of electrocity

A

Electricity the delocalised electrons Carey the charge good example is copper
Delocalised electrons are good to absorb heat energy which gives them kinetic energy which is transferred through the metals by these electrons

Science 2024 (10 decks)

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