Chemistry Quiz on Reactivity and Properties

Why are alkali metals more reactive than alkaline earth metals?

• They have a lower melting point

• They lose one electron more easily than two

• They are denser

• They are in Group 1

Why does the reactivity of halogens decrease as you go down Group 17?

• The number of valence electrons decreases

• The atomic size increases, making it harder to gain an electron

• They become more metallic

• Their ionization energy increases

Why are noble gases unreactive?

• They have a high atomic mass

• They have a stable electron configuration with a full outer shell

• They do not contain protons

• They are liquids at room temperature

Why is hydrogen placed in Group 1 despite being a non-metal?

• It has one electron in its outer shell like alkali metals

• It has similar chemical properties to Group 2 elements

• It is a gas like noble gases

• It forms double bonds

Which of the following best explains the trend in atomic radius across a period?

• Atomic radius decreases due to increased nuclear charge

• Atomic radius increases because more shells are added

• Atomic radius remains constant

• Atomic radius decreases because electrons are lost

What determines the chemical reactivity of elements?

• The number of protons

• The number of neutrons

• The number of valence electrons

• The density of the element

Why are transition metals often used as catalysts?

• They have variable oxidation states

• They are highly reactive

• They are non-conductors

• They have low melting points

Why do non-metals have higher ionization energies than metals?

• They have fewer electrons

• They are lighter

• They hold their electrons more tightly due to high nuclear charge

• They are gases

Why do elements in the same period show increasing electronegativity across the table?

• Their atomic size increases

• Their nuclear charge increases

• Their valence electrons decrease

• They have more protons

Which property explains why metals are malleable and ductile?

• Metallic bonding allows atoms to slide over each other

• They have a low density

• They have variable oxidation states

• They are conductive