Atomic structure
Name the three types of subatomic particles.
protons
neutrons
electrons
The periodic table is arranged in order of increasing....?
atomic number
Group 2 alkali earth metals would form an ion with what charge?
2+
Name 3 different types (classifications) of reactions.
Combination (composition)
Decomposition
Single displacement
Double displacement or precipitation
concentration
pressure
temperature
catalyst
surface area
If an element has an atomic number of 7 and a mass number of 15, how many protons, neutrons and electrons does it have?
7 protons
7 electrons
8 neutrons
Non-metals
Write the ion to represent Nitrogen (N). You may use your periodic table.
N3-
1. The production of ammonia (NH3) from nitrogen (N2) and hydrogen (H2) gas would be classified as what type of reaction?
2. Why is ammonia useful?
combination or composition
fertilizer
Describe collision theory.
Collision theory states that for a reaction to be successful, the reactant particles must collide, with sufficient energy and at the correct orientation.
Determine the electron configuration of phosphorus (P). You can use your periodic table.
Phosphorus has an atomic number of 15 so its configuration is 2,8,5
Describe what happens to atomic radii as you move down a group of the periodic table.
atomic radius increases (because extra electron shells are added - the period represents the number of electron shells)
Describe 2 properties of ionic compounds like salt (NaCl)
high melting point
brittle
conducts electricity only when molten or aqueous
When hydrogen gas reacts with oxygen gas in a combination reaction, water gas is formed. Write the equation in words, including states of matter.
hydrogen (g) + oxygen (g) --> water (g)
Give an example of a catalyst or enzyme and the reaction it catalyses.
Liver enzyme or manganese dioxide catalyse the decomposition of hydrogen peroxide.
Acid catalyses the decomposition of water.
UV light catalyses photosynthesis.
How many valence electrons does Neon have and why is this significant?
Neon has 8 valence electrons which makes its outer shell full. This is significant as it means the element is unreactive - it does not need to bond with another atom to be stable.
Identify the element that is shiny (lustrous) when sanded, has a high melting point, conducts electricity, and is from period 3, group 2.
Magnesium
Write the ionic formula for the compound formed between the ions Ba2+ and F-
BaF2
Explain why adding zinc or magnesium to a piece of iron helps to prevent the rusting of iron.
Zinc and magnesium are both more reactive metals than iron. This means they react preferentially with oxygen/ water and oxidise instead, thus leaving the iron protected.
Explain why increasing pressure is a way to increase the rate at which ammonia forms from nitrogen and hydrogen gas.
Pressure will only affect reactions involving gases. Since this combination reaction involves gas reactants, increasing the pressure increases the likelihood of the reactant gases colliding, thus increases the rate of ammonia production.
Identify an element with similar chemical properties to fluorine and explain what it is about their atomic structure that explains these similarities.
Any element from the same group (group 7 - halogens) would have similar chemical properties as its the number of valence shell electrons that determines how elements react. This could be Cl, Br, I
Identify which of the following elements from the same periodic of the periodic table is more electronegative: Lithium or Oxygen
Determine the correct ionic formula for potassium sulfate
Sulfate = SO42-
K2SO4
Write the formula equation for the precipitation reaction between silver (I) nitrate and sodium chloride, knowing that all cations with nitrate are soluble.
AgNO3(aq) + NaCl(aq) --> AgCl(s) + NaNO3(aq)
Explain how increasing temperature results in an increased reaction rate.
Temperature is a measure of average kinetic energy. When the kinetic energy of particles increases, the particles are moving faster, thus there will be more collisions, plus they are likely to have sufficient energy to overcome the activation energy.