GCSE Chemistry - Group 1 Alkali Metals #11

The video discusses alkali metals, highlighting their unique properties such as low density and high reactivity compared to other metals. It explains the trends in reactivity and melting points as you move down the group, emphasizing the ease of losing the outer electron. The formation of ionic compounds with non-metals is covered, along with specific reactions of alkali metals with water, chlorine, and oxygen. The video also provides examples of compounds formed and suggests using flashcards for memorization.

Which of the following is NOT a characteristic of alkali metals compared to other metals?

• High density

• Low melting point

• Softness

• High reactivity

Which alkali metal is so reactive that it can ignite spontaneously at room temperature?

• Sodium

• Lithium

• Potassium

• Cesium

Why do alkali metals become more reactive as you move down the group?

• The outermost electron is closer to the nucleus

• The atomic radius decreases

• The number of protons decreases

• The outermost electron is further from the nucleus

What happens when an alkali metal forms an ionic compound with a non-metal?

• The metal gains an electron

• The non-metal loses an electron

• The metal and non-metal share electrons

• The metal loses an electron

What type of bond is formed between sodium and chlorine in sodium chloride?

• Hydrogen bond

• Metallic bond

• Ionic bond

• Covalent bond

What is the product when sodium reacts with water?

• Sodium peroxide

• Sodium hydroxide

• Sodium oxide

• Sodium chloride

Which of the following is a possible product when potassium reacts with oxygen?

• Potassium oxide

• Potassium chloride

• Potassium superoxide

• Potassium hydroxide