WorksheetsGroup 1 Elements (Alkali Metals)
Total questions: 27
Worksheet time: 14mins
Section 1: Short Answer Questions — Select all physical properties that commonly describe Group 1 elements.
Low density compared to other metals
Soft and can be cut with a knife
Shiny when freshly cut
Good conductors of heat and electricity
High melting points
Section 1: Short Answer Questions — Why are Group 1 elements called alkali metals?
They form acidic oxides when reacting with water
They form alkaline hydroxides when reacting with water
They are found only in alkaline lakes
Their solutions are always neutral
Section 1: Short Answer Questions — Why do all Group 1 elements have similar chemical properties?
They have the same number of valence electrons
They have the same atomic masses
They have identical densities
They have identical melting points
Section 1: Short Answer Questions — Why are Group 1 metals stored in oil?
To prevent reaction with air and moisture
To improve their electrical conductivity
To keep them cool during storage
To remove impurities from the surface
Section 1: Short Answer Questions — What is the appearance of lithium, sodium, and potassium when freshly cut?
They show a shiny, silvery surface
They appear dull gray immediately
They look yellow
They turn red
Section 2: Trend-Based Questions — Select the correct trends as you go down Group 1 (from lithium to francium).
Melting point decreases
Boiling point decreases overall
Density increases overall
Reactivity increases
Atomic radius decreases
Section 2: Trend-Based Questions — Why do Group 1 metals become more reactive as you go down the group?
The outer electron is farther from the nucleus and more shielded, so it is lost more easily
Their electronegativity increases strongly down the group
More protons make a stronger attraction to the outer electron
They become less metallic down the group
Section 2: Trend-Based Questions — What is the trend in hardness of Group 1 elements from top to bottom?
They become softer down the group
They become harder down the group
Hardness stays the same
Section 2: Trend-Based Questions — How would rubidium react with water compared to lithium and potassium?
More vigorously than potassium and much more than lithium
About the same as lithium
Less vigorously than lithium
It does not react with water
Section 2: Trend-Based Questions — Why do Group 1 metals lose their outer electron easily?
They have low ionization energies due to larger atomic radius and increased shielding
They have many valence electrons to lose
They experience very strong nuclear attraction to the outer electron
They are gases at room temperature
Section 3: Reactions & Word Equations — Choose the correct word equation for the reaction of lithium with water.
Lithium + water → lithium hydroxide + hydrogen
Lithium + water → lithium oxide + oxygen
Lithium + water → lithium chloride + hydrogen
Lithium + water → lithium hydride + water
Section 3: Reactions & Word Equations — Choose the correct word equation for the reaction of sodium with water.
Sodium + water → sodium hydroxide + hydrogen
Sodium + water → sodium oxide + oxygen
Sodium + water → sodium chloride + hydrogen
Sodium + water → sodium sulfate + hydrogen
Section 3: Reactions & Word Equations — Choose the correct word equation for the reaction of potassium with water.
Potassium + water → potassium hydroxide + hydrogen
Potassium + water → potassium oxide + oxygen
Potassium + water → potassium chloride + hydrogen
Potassium + water → potassium carbonate + hydrogen
Section 3: Reactions with Water — Write a general word equation for a Group 1 metal reacting with water.
Group 1 metal + water → metal hydroxide + hydrogen
Group 1 metal + water → metal oxide + oxygen
Group 1 metal + water → metal carbonate + carbon dioxide
Group 1 metal + water → metal chloride + chlorine
Section 3: Reactions with Water — What two products are formed when an alkali metal reacts with water?
A metal hydroxide and hydrogen gas
A metal carbonate and carbon dioxide
A metal oxide and oxygen gas
A metal chloride and chlorine gas
Section 3: Reactions with Water — Write the balanced chemical equation for sodium reacting with water.
2Na + 2H2O → 2NaOH + H2
Na + H2O → Na2O + H2
2Na + H2O → Na2O + H2O
Na + 2H2O → NaOH + H2O
Section 3: Reactions with Water — What are signs that a chemical reaction is taking place when potassium is added to water?
Fizzing and a lilac flame are observed
No temperature change and the metal remains still
The solution becomes clear without gas production
A white precipitate forms with no heat released
Section 4: Gases & Tests — What gas is produced when a Group 1 metal reacts with water?
Hydrogen
Oxygen
Chlorine
Carbon dioxide
Section 4: Gases & Tests — How can you test for hydrogen gas in the lab?
Apply a lit splint to the gas and listen for a squeaky pop
Bubble the gas through limewater to turn it milky
Hold damp blue litmus over the gas to turn it red
Use a glowing splint and look for relighting
Section 4: Gases & Tests — Why does the reactivity with water increase from lithium to cesium?
The outer electron is lost more easily due to increased atomic radius and shielding
The atoms become smaller and hold electrons more tightly
Ionization energy increases down the group
There are fewer electron shells down the group
Section 4: Gases & Tests — A student sees fizzing and a lilac flame when adding a metal to water. Which Group 1 element was likely used?
Lithium
Sodium
Potassium
Rubidium
Section 5: Extension & Application — Compare the reaction of calcium (Group 2) with water to that of sodium.
Calcium reacts more slowly than sodium, producing calcium hydroxide and hydrogen, while sodium reacts more vigorously to form sodium hydroxide and hydrogen
Calcium reacts more vigorously than sodium and produces oxygen gas, while sodium produces chlorine gas
Both react at the same rate and produce identical flame colors
Neither reacts with water under normal conditions
Section 5: Extension & Application — Why are Group 1 elements not found freely in nature?
They are highly reactive and readily form compounds
They are too rare to exist in Earth’s crust
They are gases at room temperature
They dissolve completely in water
Section 5: Extension & Application — What safety precautions should be taken when handling Group 1 metals? Select all that apply.
Wear goggles and use a safety screen
Cut small pieces and handle with tongs
Store the metals under oil away from water
Add large chunks directly to water for clearer results
Section 5: Extension & Application — How could you experimentally compare the reactivity of lithium, sodium, and potassium?
Add equal-sized pieces to water and measure the rate of hydrogen production or time to disappear
Heat each metal strongly in air and compare the oxide masses
Weigh equal volumes of the metals and compare densities
Dissolve each metal in ethanol and record the temperature change
Section 5: Extension & Application — What would you expect to observe if cesium was dropped into water?
An extremely violent reaction with rapid hydrogen production, heat, and possible explosion
A slow reaction with gentle bubbling and no heat
No visible reaction at room temperature
Formation of a white precipitate without gas
Section 5: Extension & Application — Why are Group 1 elements used in fireworks?
They produce characteristic flame colors useful for pyrotechnic effects
They make fireworks heavier and more stable in flight
They prevent moisture from affecting the fuses
They react to absorb heat and cool the display
