Fichas
Formulae and equations
Fichas del conjunto (14)
- 1What are the seven diatomic elements?Iodine
Bromine
Chlorine
Fluorine
Oxygen
Nitrogen
Hydrogen - 2What is a diatomic elementElements which exist only as molecules of two atoms.
- 3What are the charges of the ions: bromide, carbonate, chloride, fluoride, hydroxide, iodide, nitrate, oxide, sulfate?Bromide: Br -
Carbonate: CO3 2-
Chloride: Cl -
Fluoride: F -
Hydroxide: OH -
Iodide: I -
Nitrate NO3 -
Oxide: O 2-
Sulfate:
SO4 2- - 4What are the charges of the ions: aluminium, ammonium, barium, calcium, copper (II), hydrogen, iron (II), iron (III)?Aluminium: Al 3+
Ammonium: NH4 +
Barium: Ba 2+
Calcium: Ca 2+
Copper (II): Cu 2+
Hydrogen: H +
Iron(II): Fe 2+
Iron (III): Fe 3+ - 5What are the charges of the ions: lithium, magnesium, nickel, potassium, silver, sodium, zinc?Lithium: Li +
Magnesium: Mg 2+
Nickel: Ni 2+
Potassium: K +
Silver: Ag +
Sodium: Na +
Zinc: Zn 2+ - 6What are the oxidation number rules?1. Uncombined elements are 0
2. Sum of all atoms/ions in a neutral compound is 0
3. Sum of all atoms in an ion is equal to the ion's charge
4. More electronegative element in a substance is negative and less electronegative is positive
5. Fluorine is always -1
6. Oxygen is usually -2
7. Hydrogen is usually +1
8. In compounds, groups 1, 2 and aluminium are +1, +2 and +3 respectively - 7What are the first two most electronegative elements?1. fluorine
2. oxygen - 8What are the exceptions to the rules of oxidation numbers?1. Hydrogen in a metal hydride (combined with only metal) is -1
2. Oxygen is +2 when combined with F and -1 when in a peroxide
3. Chlorine is not -1 when combined with fluorine/oxygen - 9Give the definitions of oxidation and reductionOxidation: when something loses electrons
Reduction: when something gains electrons - 10Give the definitions of oxidation number and standard stateOxidation number: number showing the number of electrons lost/gained by an atom of that element in a compound.
Standard state: an element that exists at 25 degrees celcius - 11Give the definitions of spectator ion, total ionic equation and net ionic equationSpectator ion: Ion that is present in solution but doesn't participate in the precipitation reaction.
Total ionic equation: before the spectator ions have been removed.
Net ionic equation: after the spectator ions have been removed. - 12What are the steps to writing a net ionic equation?1. Balance the molecular equation
2. Split aqueous compounds into ions with charges
3. Cancel out the spectator ions - 13Oxidation numberNumber of electrons that need to be added to or taken away from an element to make it neutral
- 14When are oxidation numbers used?Used in redox reactions to show which species is oxidised & which is reduced.
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- Descripción
- AS level Chemistry Fichas sobre Formulae and equations, creado por Bethan Lewis el 13/09/2016.
- Creado por
- Bethan Lewis
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