1) What is a covalent bond? a) Shared electrons b) Transferred electrons c) Metallic bond d) Ionic bond 2) Which bond is strongest? a) Ionic bond b) Covalent bond c) Hydrogen bond d) Van der Waals 3) What is solubility? a) Dissolving ability b) Melting ability c) Boiling ability d) Freezing ability 4) Polar substances are: a) Non-polar b) Have dipoles, either positive or negative c) Neutral d) Ionic 5) Non-polar substances: a) Have no dipoles b) Have dipoles c) Are ionic d) Are polar 6) What are electrical insulators? a) Conduct electricity b) Block electricity c) Are metals d) Are ionic 7) Why do molecular substances usually have low melting and boiling points? a) They are held together by weak intermolecular forces b) They have tightly packed atoms like metals c) They contain strong metallic bonds d) They are always ionic 8) Why do molecular substances not conduct electricity in solid form? a) Electrons are delocalized and free to move b) They have strong metallic bonds c) They have high melting points d) There are no free electrons or ions to carry current 9) Why is water a liquid at room temperature while sodium chloride is solid? a) Sodium chloride has weak metallic bonds b) Water has metallic electrons that hold molecules together c) Water has strong covalent bonds but weak intermolecular forces d) Sodium chloride is a liquid at high temperatures 10) Why do molecular substances like sugar dissolve easily in water? a) Because sugar contains metallic bonds b) Because sugar molecules are ionic c) Because sugar is non-polar d) Because polar molecules interact with polar water molecules 11) Why are molecular substances often soft or brittle? a) Covalent bonds always allow flexibility b) Weak intermolecular forces break easily when force is applied c) They contain ionic lattices d) Strong metallic bonds make them hard 12) Why do molecular substances usually not conduct electricity in solution? a) Their covalent molecules do not break into ions b) They form metallic bonds when dissolved c) They contain free electrons in solution d) They are always ionic in solution 13) Why are molecular substances often gases at room temperature? a) Strong intramolecular forces hold them apart b) They contain metallic bonding c) Weak intermolecular forces allow molecules to separate easily d) They contain free ions 14) Why does diamond not conduct electricity while graphite does? a) Graphite is softer than diamond b) Diamond’s electrons are all used in covalent bonds, graphite has delocalized electrons c) Diamond has free electrons, graphite does not d) Diamond has metallic bonds 15) Which bond involves electron transfer? a) Ionic bond b) Covalent bond c) Metallic bond d) Hydrogen bond 16) Why is methane a gas at room temperature? a) Because CH₄ molecules are small with weak intermolecular forces b) Because it is metallic c) Because CH₄ has strong ionic bonds d) Because it is polar 17) Why does molecular iodine have a low melting point compared to sodium chloride? a) Weak intermolecular forces between I₂ molecules require little energy to break b) Iodine contains metallic bonds c) Iodine has ionic bonds d) Sodium chloride is soft 18) Why can molecular substances be brittle solids? a) Covalent bonds allow flexibility b) Strong metallic bonds resist bending c) Ionic lattices make them flexible d) Weak intermolecular forces break easily under stress 19) Why does ethanol dissolve in water? a) It is non-polar and repels water b) Ethanol has metallic bonding c) Polar O-H bonds interact with polar water molecules d) Ethanol contains free ions 20) Why do molecular gases like oxygen and nitrogen have low boiling points? a) Weak van der Waals forces between molecules require little energy to overcome b) They have metallic electrons c) Strong covalent bonds hold them together in gas phase d) They are ionic compounds 21) Why do molecular substances have low density compared to metals? a) Intermolecular forces push molecules close together b) Molecular substances contain metallic bonds c) Molecular substances are ionic d) Molecules are small and loosely packed 22) Why does molecular sulfur not conduct electricity? a) Sulfur contains metallic bonds b) All electrons are involved in covalent bonds, so no free charges exist c) Sulfur is soluble in water d) It contains delocalized electrons 23) Why are molecular substances poor conductors even when dissolved? a) Free electrons in molecules carry charge b) Intermolecular forces create current c) Covalent molecules do not break into ions in solution d) Metallic bonding allows conduction 24) Why do molecular substances like carbon dioxide and methane not conduct electricity in any state? a) All their electrons are involved in covalent bonds, so no charged particles are available to carry current b) They have free electrons that move too slowly c) They are always solids at room temperature d) They contain metallic bonds that block current 25) Why do molecular substances like wax or sugar melt easily compared to metals? a) They contain free electrons that carry heat away b) Strong covalent bonds within molecules are easy to break c) They are magnetic and attract heat d) Only weak intermolecular forces need to be overcome for melting

Chemistry: Bonding and Properties

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