18 Questions
What is the product of the thermal decomposition of barium carbonate?
Barium sulfate
Why do Group 1 metals tend to have low melting points?
Weak metallic bonding
Which property decreases down Group 1 in the periodic table?
Ionization energy
What makes the outer electrons of Group 2 metals easier to lose down the group?
Increased atomic radius and shielding
Which Group 2 metal is most likely to react most vigorously with water?
Beryllium
What property of Group 2 metals allows them to form 2+ ions when they react?
The loss of two electrons
Why do Group 1 metals produce different colors in flame tests?
As a result of electron transitions when energy is absorbed
Which Group 2 metal compound produces a crimson red color in flame tests?
Strontium
What is the color observed when barium compounds are subjected to a flame test?
Green
Why do halogens gain an electron to form a 1- ion?
To achieve a full outer shell
What trend is observed in the atomic radius of Group 7 elements?
Increases down the group
In thermal decomposition reactions, what happens to Group 2 metal compounds?
They release energy in the form of light
What is the product of the thermal decomposition of magnesium hydroxide?
Magnesium oxide
Which of the following is a property of group 2 metals?
They can form metal peroxides with excess oxygen and heat energy
Which of the following group 1 metals can react with excess oxygen to form metal peroxides?
Cesium
What type of reaction occurs when group 2 hydroxides react with dilute acid?
Neutralization reaction
When group 2 metals react with dilute acids, what is one of the products formed?
Salt and hydrogen gas
What color precipitate is formed when group 2 metals react with chlorine gas?
White
Study Notes
Reactions of Magnesium
- Magnesium is oxidised from an oxidation state of 0 to +2
- Magnesium reacts slowly with liquid water, but faster with steam, producing a bright white flame and forming hydrogen and magnesium oxide, a white powder
Reactions of Group 2 Metals
- Group 2 metals react with chlorine gas to form metal chlorides, which are all white precipitates
- The reactions become more vigorous down the group as the elements are more reactive
- Group 2 metals react with oxygen to form oxides, which can be vigorous
- Strontium and barium can react with excess oxygen and heat energy to form metal peroxides
- Group 2 metals react with dilute acids to produce bubbles of hydrogen gas and solutions of metal compounds
- Group 2 hydroxides react with dilute acid to form a salt and water, a type of neutralisation reaction
Properties of Group 2 Elements
- Group 2 metals react by losing two electrons to form 2+ ions, achieving a full outer shell
- Atomic radius of Group 2 metals increases down the group due to additional electron shells
- Reactivity of Group 2 metals increases down the group due to increased electron shielding and atomic radius
- First ionisation energy of Group 2 metals decreases down the group due to a greater atomic radius and increased shielding
Flame Tests
- The colours observed in the flame tests of Group 1 and Group 2 metal compounds are due to electron transitions
- The colour produced depends on the wavelength of the light energy emitted
- Not all atoms and ions produce a colour in the flame test as the energy emitted may not have a wavelength in the visible light part of the electromagnetic spectrum
Trends in Halogen Properties
- Group 7 elements are highly reactive non-metals
- Atomic radius of Group 7 elements increases down the group due to additional electron shells
Learn about the elements of Group 1 & 2 in Inorganic Chemistry and the Periodic Table with detailed notes from PMT Education. Understand how Group 2 elements form 2+ ions by losing two electrons. Explore the physical properties of these elements.
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