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CHEMISTRY > Foundations In Chemistry > Flashcards

Foundations In Chemistry Flashcards

1
Q

State the 3 sub atomic particles their properties

A

Protons
relative charge +1
relative mass 1

Neutrons
Relative charge 0
Relative mass 1

Electrons
Relative charge -1
Relative mass 1/2000 (negligible)

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2
Q

Define isotope

A

Atoms of the same element which have different numbers of neutrons

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3
Q

Define relative atomic mass

A

The weighted mean mass of an atom of an element compared to 1/12 the mass of a carbon 12 atom

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4
Q

Define relative isotopic mass

A

The mass of an atom of an isotopes compared to 1/12 of a carbon 12 atom

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5
Q

Define ion

A

An ion is an atom that has a charge due to gaining or losing an electron(s)

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6
Q

What is the mass number and atomic number

A

Mass number (the biggest number-MASSive) is equal to the number of protons+neutrons in the nucleus

Atomic number is equal to the number of protons in the nucleus (also equal to the number of protons in ATOMS NOT IONS)

To find the number of neutrons you subtract the atomic number from the mass number

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7
Q

What is the calculation for relative atomic mass?

A

RAM= (abundance 1 x isotopic mass 1) + (abundance 2 x isotopic mass 2) / 100

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8
Q

Define shells, sub shells and orbitals

A

Shells- a shell is a group of atomic orbitals with the same principle quantum number (shell number). The shell closest to the nucleus has a number of 1 and has the lowest energy.

Sub shells- a group of the same type of atomic orbitals within a shell (s, p, d, f)

Orbitals- a region in atom around the nucleus which can hold up to two electrons with opposite spins.

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9
Q

Describe the shape of s and p orbitals

A

S orbitals- spherical shape
P orbitals- dumbbell shape

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10
Q

Describe the filling of atomic orbitals

A

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6

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11
Q

What is the electron configuration for chromium (24 e-) and copper (29 e-)?
Why are they like this?

A

Chromium: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^5

Copper: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^10

This is because they are more stable this way

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12
Q

How do u draw the filling of atomic orbitals?

A

Boxes with arrows (you don’t want stinky people next to you)

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13
Q

In what order do electrons fill orbitals?

A

Electrons fill from the lowest energy level orbitals first up to the highest energy level orbitals last

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14
Q

Why is X classed as an (s/p/d/f) block element?

A

Because it’s highest energy level electron occupies an (s/p/d/f) orbital

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15
Q

Define transition elements

A

A d Block Element which forms an ion with an incomplete d sub shell

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16
Q

What do transition elements lose first when forming positive ions?

A

4s electrons

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17
Q

Define empirical formulae

A

The simplest whole number ratio of elements in a compound

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18
Q

How do you calculate empirical formulae

A

Calculating Empirical Formula:
1. Determine the mass of each element in the compound.
2. Convert the masses to moles using the relative atomic masses.
3. Divide the moles of each element by the smallest number of moles to get the ratio.
• Example: For a compound containing 6.0 g of carbon and 8.0 g of hydrogen, the moles of carbon and hydrogen are calculated, and the ratio is used to find the empirical formula.

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19
Q

Define molecular formulae

A

The actual number of atoms of each element in a molecule

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20
Q

How do you calculate molecular formulae

A

The molecular formulae can be determined if the relative atomic mass of the compound is known:
• Formula: molecular formulae = Empirical formula x n
• Where n is the ratio of the molar mass of the compound to the empirical formula mass.

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21
Q

What are the rules for metal ions, non metal ions and transition metal ions

A

Metal ions: +ve ions usually ending in -ium

Non-metal ions: -ve ions usually ending in -ide, (-ate or -ite which mean containing oxygen)

Transition metals: +ve ions of variable charge

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22
Q

What is an ionic compound and how do you write them

A

Consist of oppositely charged ions held together by electrostatic forces

-Identify the charges on the ions.
-Balance the charges to form a neutral compound via the crossover method

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23
Q

Name the different compound ions

A

OH (-)
NO3 (-)
MnO4 (-)
CO3 (2-)
SO4 (2-)
SO3 (2-)
Cr2O7 (2-)
PO4 (3-)

24
Q

How do you write chemical equations

A

-Write the equation in words
-Put in all the state symbols and chemical formulae
-Balance the equation

25
Q

Define acid

A

An acid is a proton or H+ donor. They release H+ ions in an aqueous solution.

26
Q

Explain the difference between a strong and weak acid

A

Strong Acids: Completely dissociate in aqueous solutions, releasing all its acidic hydrogen atoms

Weak Acids: Only partially dissociate in aqueous solutions, releasing some but not all of its acidic hydrogen atoms

27
Q

Define base and list some types

A

A base is a proton or H+ acceptor.

Types:
Metal oxide
Metal hydroxide
Metal carbonate
Ammonia solution

28
Q

Define an alkali

A

An alkali is a base that dissolves in water and releases OH- ions in aqueous solutions

29
Q

Define a salt

A

A salt is produced when the H+ ion of an acid is replaced by a metal or NH4+

It is produced from the neutralisation of an acid and a base

30
Q

Explain the reactions to make a salt

A

Acid + ammonia = ammonium salt

Acid + metal oxide = salt + water

Acid + metal hydroxide = salt + water

Acid + metal = salt + hydrogen

Acid + metal carbonate = salt + water + carbon dioxide

31
Q

Explain the solubility of salts

A

-All sodium, potassium, and ammonium salts are soluble.
-Most chloride salts are soluble, except for silver chloride and lead(II) chloride.
-Most sulfate salts are soluble, except for barium sulfate and calcium sulfate.

32
Q

Explain the properties of a salt

A

Salts are generally crystalline and have high melting and boiling points due to the strong ionic bonds.

Salts like sodium chloride can conduct electricity when molten or dissolved in water because the ions are free to move.

33
Q

Explain what a standard solution is and how to produce one

A

A standard solution is a solution of known concentration

To prepare it:

-Accurately weigh the solid (mass by difference method)
-Dissolve the solid in a beaker using a small amount of distilled water
-Carefully transfer the solution into the volumetric flask. Ensure you rinse the
beaker with distilled water and add this to the volumetric flask.
-Carefully fill the flask with distilled water until the bottom of the meniscus
lines up exactly with the graduation mark
-Invert the flask several times (with the stopper fitted) to mix the solution.

34
Q

Explain how to carry out an acid-base titration

A

-25.0cm3 of the solution A was transferred into a conical flask using a pipette
-Indicator was added to the solution in the conical flask
-Solution B of unknown concentration was added to the burette and the initial
burette reading was recorded to the nearest 0.05cm3
-The solution B was slowly added to the conical flask until the indicator
changed colour at the end point.
-The final burette reading was recorded to the nearest 0.05cm3
-The titration was then repeated until two concordant results were achieved
-record the data in a table, containing the initial volume, final volume and titre

35
Q

What is an acid base titration used for

A

To find the concentration of a solution of unknown concentration from a solution of a known concentration

36
Q

How do you calculate the unknown concentration

A

Concentration 1 x volume 1 = concentration 2 x volume 2 (given the units are the same)

This is because the moles are the same because there is an equal number of moles of acid to moles of the base which is why it becomes neutralised

37
Q

Explain what moles are

A

A mole is an amount of a substance which is equivalent to the number of atoms in 12g of carbon 12 or 6.02x10^23 particles (atoms, molecules etc)

38
Q

How do you calculate moles

A

Moles=mass/mr

39
Q

Explain molar mass

A

The mass in grams per mole of a substance

40
Q

How do you calculate number of particles

A

Number of particles = moles x Avagadros constant

41
Q

How do you calculate moles of a substance using stoichiometric ratios

A

-Write a Balanced Chemical Equation. Ensure the equation is balanced before starting calculations.
-Identify the Known and Unknown
-Use the Mole Ratio from the balanced equation, determine the stoichiometric relationship between the known and unknown substances
-Perform Calculations. Convert given quantities (mass, volume, concentration) into moles if necessary.
-Use the mole ratio to calculate the number of moles of the unknown substance.
-Convert moles back to required units (mass, volume, etc.) if needed.

42
Q

How do you calculate moles in a solution

A

Moles = concentration x volume (divide by 1000 if one of the units is in cm3 or by 1000000 if both are in cm3)

43
Q

How do you calculate moles of a gas

A
44
Q

Explain percentage yield and how to calculate it

A

Percentage yield measures the efficiency of a chemical reaction by comparing the actual yield of a product to the theoretical yield

Percentage yield = actual yield/theoretical yield (x100)

45
Q

Explain why you may have a low yield

A

-Incomplete reactions (not all reactants react).
-Side reactions (producing unwanted by-products).
-Loss of product during purification or transfer.
-Reversible reactions not going to completion.

46
Q

Explain atom economy and how to calculate it

A

Atom economy measures the proportion of reactants that are converted into useful (desired) products. It evaluates the sustainability and efficiency of a chemical reaction.

Atom economy = Mr of desired products/Sum of Mr of all reactants (x100)

47
Q

Explain why atom economy is relevant

A

-Atom economy indicates how much waste a reaction produces.
-Reactions with high atom economy are more sustainable and environmentally friendly
-Higher atom economy reduces waste and improves efficiency, making industrial processes more sustainable

48
Q

Explain how to maximise atom economy

A

-Use reactions where most/all reactants become the desired product.
-Reactions with fewer by-products have higher atom economies.

49
Q

Explain the difference between atom economy and percentage yield

A

Percentage yield focuses on the actual efficiency of producing the product compared to theoretical amounts whereas atom economy focuses on the proportion of reactants that end up in the desired product, regardless of losses or inefficiencies

50
Q

Explain what oxidation and reduction are

A

Oxidation is a loss of electrons and reduction is the gain of electrons

51
Q

Explain what an oxidising agent is and what a reducing agent is

A

Oxidising agents accept electrons and get reduced
Reducing agents donate electrons and get oxidised

52
Q

What are the general rules for oxidation numbers

A

-Uncombined elements + HONClBrIF = 0
-ions = charge of the ion
-Hydrogen = +1 unless in a metal hydride where its -1
-Oxygen = -2 unless in peroxides where its -1 or bonded to fluorine where its +2

53
Q

How do you find the oxidation state of an element in a compound

A

Start with the most electronegative and progress down until you finish with all your known oxidation states. Then assign an appropriate oxidation state, accounting for the charge of the compound

54
Q

How do you identify what is being oxidised or reduced

A

Oxidation: increase in oxidation number
Reduction: decrease in oxidation number

55
Q

How do you write a half equation

A

-Identify species being oxidised or reduced
-Balance atoms (except H and O)
-Balance oxygen using H₂O
-Balance hydrogen using H⁺ ions
-Balance charge using electrons (e⁻)

56
Q

How do you combine half equations

A

-Ensure the number of electrons in oxidation and reduction half-equations are equal
-Add the two half-equations together and cancel electrons
-simplify

57
Q

What is the term for when a substance is oxidised and reduced simultaneously

A

Disproportionation

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