Introduction to Group 7 Elements: The Halogens

The video tutorial explores group 7 elements, known as halogens, focusing on their electronic structure, reactivity, and properties. Halogens have seven electrons in their outer shell, making them highly reactive, especially with metals, forming salts. The reactivity decreases down the group due to increased electron shells. Halogens exist as diatomic molecules and can form hydrogen halides, which are acidic in water. Displacement reactions occur when more reactive halogens displace less reactive ones. The video also discusses the physical properties of halogens, such as melting and boiling points, which increase down the group.

What is the electronic structure of halogens in their elemental form?

• Tetratomic molecules with a quadruple covalent bond

• Diatomic molecules with a single covalent bond

• Monatomic molecules with a double covalent bond

• Triatomic molecules with a triple covalent bond

What type of compound is formed when halogens react with metals?

• Metal nitrates

• Metal sulfides

• Metal halides

• Metal oxides

Why are halogens more reactive at the top of their group?

• They have fewer electron shells, increasing nuclear attraction

• They have more electron shells, decreasing nuclear attraction

• They have a higher atomic mass, increasing reactivity

• They have a lower atomic mass, decreasing reactivity

What happens when hydrogen halides are dissolved in water?

• They form alkaline solutions

• They form basic solutions

• They form neutral solutions

• They form acidic solutions

Which halogen is most likely to displace another from a halide solution?

• A halogen with a lower atomic number

• A less reactive halogen

• A halogen with a higher atomic number

• A more reactive halogen

As you move down the group of halogens, what happens to their melting and boiling points?

• They fluctuate randomly

• They increase

• They remain constant

• They decrease

How can the properties of unknown halogens be predicted?

• By using the properties of noble gases

• By using the properties of alkali metals

• By using the properties of other halogens

• By using the properties of transition metals