Chemistry paper 1 c1-7 Flashcards
Name the 3 subatomic particles
Protons, neutrons, electrons
Name the 2 subatomic particles in the nucleus
Protons and neutrons
Give the location of electrons in the atom
Orbiting the nucleus in shells
Give the maximum number of electrons in the first shell
Maximum of 2
Give the maximum number of electrons in the second and third shells
Maximum of 8
Give the charge of a proton
Positive (+1)
Give the charge of a neutron
Neutral (0)
Give the charge of an electron
Negative (-1)
Explain why the overall charge of an atom is zero
Same number of protons and electrons
Define an atom
Smallest particle that makes up all matter
Define an element
Substances made from only one type of atom
Define a compound
Substances made from two or more types of atoms bonded together
Define a mixture
Groups of atoms, elements and compounds that are mixed but not bonded
Define an ion
Charged particle formed when an atom has lost or gained electrons
Define an isotopes
Atoms of the same element (same number of protons) with a different number of neutrons
Name the process to separate two liquids
Distillation
Name the process to separate an insoluble solid from a liquid
Filtration
Name the process to separate a soluble solid from a liquid
Crystallisation
Name the four scientists involved in the development of the periodic table
John Dalton, John Newlands, Dimitri Mendeleev, Henry Moseley
Describe the contribution of Dalton to develop the periodic table
Ordered elements based on their atomic mass
Describe the contribution of Newlands to develop the periodic table
Kept atomic mass. Discovered a repeating pattern every 8th element
Describe the contribution of Mendeleev to develop the periodic table
Switched positions of elements that did not fit patterns. Left gaps for undiscovered elements
Describe the contribution of Moseley to develop the periodic table
Ordered elements based on the number of protons they had
Give the properties of alkali metals
Very reactive, low melting/boiling points, react vigorously with water and halogens
Give the properties of the halogens
Low melting/boiling points, poor conductors of heat/electricity, toxic, react with alkali metals
Give the properties of noble gases
Very unreactive, stable, full outer shell, exist as single atoms
Identify the pattern of reactivity in group 1 (Alkali metals)
The Alkali metals become more reactive as you go down the periodic table
Identify the pattern of reactivity in group 7 (Halogens)
The Halogens become less reactive as you go down the periodic table
Give the word equation for the reaction between an alkali metal and water
Alkali metal + water → Alkali metal hydroxide + hydrogen
Define a displacement reaction
When a more reactive element takes the place of a less reactive element in a compound
List the three types of bonding
Ionic, covalent, metallic
State the type of bonding that occurs between metals
Metallic
State the type of bonding that occurs between non-metals
Covalent
State the type of bonding that occurs between metals and non-metals
Ionic
Describe what happens in ionic bonding
Electrons are lost or gained
Describe what happens during covalent bonding
Electrons are shared
List the properties of solids
Fixed shape, fixed volume, cannot be compressed, particles arranged in rows, particles vibrate in fixed positions
List the properties of liquids
Can change shape, fixed volume, cannot be compressed, particles not arranged in rows, particles can slide past each other
List the properties of gases
Can change shape, can change volume, can be compressed, particles arranged randomly, particles move freely in all directions
Describe the properties of ionic compounds
High melting and boiling points, conducts electricity when molten/dissolved, brittle
Give the structure that ionic compounds form
Giant lattices
Explain why ionic compounds have high melting/boiling points
Strong electrostatic forces between oppositely charged ions, lots of energy needed to overcome them
Explain why simple covalent molecules have low melting/boiling points
Weak intermolecular forces between molecules, these are easily overcome
State the material that diamond, graphene and graphite are made from
Carbon atoms
List the properties of diamond
Hard, strong, cannot conduct electricity
Explain why diamond is hard and strong
Forms 4 covalent bonds per atom. This is the max number of bonds. Lots of energy required to break them
Describe the structure of Graphene
2D sheet of carbon atoms arranged in hexagons
Describe the structure of graphite
3D structure made from multiple graphene layers
List the properties of graphite
Soft, brittle, can conduct electricity, 3D
Explain why graphite is soft
Graphite has layers. There are weak forces between layers. These layers can slide over each other
Explain why graphite can conduct electricity
Only forms 3 bonds per atom. This means there is 1 spare electron that can conduct electricity
List the properties of metals
High melting/boiling points, conduct electricity, malleable
Describe the structure of metals
Positive metal ions. A sea of delocalised electrons. Strong electrostatic forces between them
Define atomic number
The number of protons in the nucleus of an atom
Define mass number
The number of protons PLUS the number of neutrons
Define isotope
Isotopes have the same number of protons but a different number of neutrons
Define relative formula mass
The mass of a molecule
Describe how to calculate relative formula mass
Add up all the relative atomic masses of each atom in the molecule
State how to calculate % by mass
(Ar of the element / Mr of the compound) x 100
State the equation for calculating concentration
Concentration = mass / volume
State the units for concentration
g/dm3
Describe how to convert from cm3 to dm3
Divide by 1000
Describe how to convert from dm3 to cm3
Times by 1000
Define the reactivity series
List of metals in order of reactivity
Name the metals that can be extracted using carbon
Zinc, iron, tin, lead, copper, silver, gold, platinum
Name the metals that can only be extracted using electrolysis
Potassium, sodium, calcium, magnesium, aluminium
Define displacement reaction
When a more reactive metal takes the place of a less reactive metal
Give the general word equation for the reaction between a metal and oxygen
Metal + Oxygen → Metal oxide
Give the general word equation for the reaction between a metal and acid
Metal + acid → salt + hydrogen
Give the general word equation for the reaction between a metal oxide and carbon
Metal oxide + carbon → Metal + carbon dioxide
Give the general word equation for the reaction between an acid and a base
Acid + base → Salt + water
Give the general word equation for the reaction between a metal carbonate and acid
Metal carbonate + acid → Salt + water + carbon dioxide
Give the general word equation for the reaction between a metal and water
Metal + water → Metal hydroxide + hydrogen
Name the salt produced by hydrochloric acid
Metal chloride
Name the salt produced by sulphuric acid
Metal sulphate
Name the salt produced by nitric acid
Metal nitrate
Define an ore
A rock that contains enough metal atoms to make extracting them commercially viable
Define oxidation
Gain of oxygen, loss of electrons
Define reduction
Loss of oxygen, gain of electrons
Define salt
An ionic compound with no overall charge
Which ion makes a substance acidic?
H+
Which ion makes a substance alkaline?
OH-
Define a base
Chemicals capable of neutralising acids
Give three examples of bases
Metal oxides, Metal hydroxides, Metal carbonates
Define an alkali
Soluble base
Define electrolysis
Splitting a compound using electricity
State the states of matter required for electrolysis to take place
Molten (melted) or aqueous (dissolved in water)
Explain why electrolysis works with molten/aqueous compounds
Ions are free to move towards the electrodes
Explain why electrolysis won’t work if the compound is solid
Ions are arranged in rows and cannot move towards the electrodes
State the type of compounds that can be split by electrolysis
Ionic compounds
State the types of elements found in ionic compounds
Made from a metal and a nonmetal
Define ion
Charged particle formed when atoms lose or gain electrons
State the type of element that forms cations
Metals
State the type of element that forms anions
Non-metals
State the name of the positive electrode
Anode
State the name of the negative electrode
Cathode
Explain which ions are attracted to the anode
Anions, since they are negatively charged and attracted to the positively charged anode
Explain which ions are attracted to the cathode
Cations, since they are positively charged and attracted to the negatively charged cathode
Explain what happens to ions at the anode
Anions lose electrons to become atoms. They are oxidised
Explain what happens to ions at the cathode
Cations gain electrons to become atoms. They are reduced
Explain why cryolite is used in the electrolysis of aluminium oxide to make aluminium
Cryolite reduces the melting point of aluminium oxide so less energy is needed to melt it
Explain why the anodes need constant replacing in the extraction of aluminium
The anodes are made of graphite. This reacts with the oxygen produced at the anode, forming carbon dioxide gas
State which ions are contributed by water in solutions of ionic compounds
Hydrogen ion H+, Hydroxide ion OH-
Explain how the product produced at the cathode during electrolysis of solutions is determined
If the metal ion from the ionic compound is more reactive than hydrogen, then hydrogen is formed. If it is less reactive, then the metal is formed
Explain how the product produced at the anode during electrolysis of solutions is determined
If the anion is a halide ion (chloride, bromide, iodide), then the halogen (chlorine, bromine, iodine) is produced. If the anion is anything else (e.g. sulfate, nitrate) then oxygen is produced
Explain how a third product of electrolysis of solutions can be made
The ions that are left behind in the solution following electrolysis form a third product
Define an exothermic reaction
An exothermic reaction is one that transfers energy from the reacting chemicals to the surrounding area
Define an endothermic reaction
An endothermic reaction is one that transfers energy from the surrounding area to the reacting chemicals
Define activation energy
The minimum energy needed for a reaction to take place
Define bond energy
The energy required to break a specific chemical bond
Define a reaction profile
The relative difference in the energy of reactants and products
Give the charge for an endothermic reaction in bond energy
positive
Give the charge for an exothermic reaction in bond energy
Positive
Give the reaction type when the energy of the products is lower than the energy of the reactants
Exothermic
Give the reaction type when the energy of the products is higher than the energy of the reactants
Endothermic
Give an example of an exothermic reaction
Fireworks, combustion, self heating cans, hand warmers
Give an example of an endothermic reaction
Thermal decomposition, ice packs
Identify if making bonds is exothermic or endothermic
Exothermic
Identify if breaking bonds is exothermic or endothermic
Endothermic
