Bonding In Elements - Higher Chemistry Unit 1

Which of the following elements is monatomic at room temperature and pressure?

• Chlorine

• Hydrogen

• Helium

• Sulfur

What are the forces of attraction that hold Argon atoms together?

• pd-pd

• LDF

• hydrogen bonding

• covalent bonds

Which of the following consists of discrete covalent molecules

• Lithium

• Boron

• Sulfur

• Magnesium

The two chlorine atoms in a molecule of chlorine are held together by

• LDF

• a polar covalent bond

• a pure covalent bond

• an ionic bond

Which of these consists of polyatomic, X₈ molecules?

• Phosphorus

• Argon

• Oxygen

• Sulfur

Which of the following does not contain covalent bonds?

• solid sulfur

• hydrogen gas

• argon gas

• oxygen gas

Why do substances such as diamond and graphite have high melting and boiling points?

• they are held together by strong hydrogen bonds

• the metallic bonds present are intramolecular forces and so therefore very hard to break

• carbon atoms in these substances are held together by strong covalent bonds

• these structures are so large that LDF forces are very strong

Why does Sulfur have a higher melting point than Phosphorus?

• Sulfur has a larger gfm and so more electrons so LDF forces are stronger and harder to break

• Sulfur has strong covalent bonds whereas Phosphorus only has LDF to break to change state

• Trick question - It doesn't! Phosphorus has a higher melting point that Phosphorus

• Sulfur has pdpd and phosphorus has LDF. Pdpd are harder to break

Which structure best describes the normal state of sodium?

• metallic lattice

• monatomic gas

• molecular solid

• molecular gas

Which of the following best describes the normal state of a fullerene?

• covalent network

• metallic lattice

• covalent molecule

• monatomic gas