A) Sulphur and oxygen B) Carbon and oxygen C) Nitrogen and oxygen D) Oxygen and hydrogen
A) XY2 B) X3Y2 C) X2Y D) X2Y3
A) 6 and 2 B) 2 and 3 C) 1 and 3 D) 8 and 2
A) +7 B) -5 C) +8 D) -7
A) Crystallisation B) Sublimation C) Evaporation D) Melting
A) Potassium B) Chlorine C) Argon D) Sulphur
A) Electrons between two atoms B) Protons between two atoms C) Neutrons between two atoms D) Electrons from one atom to another
A) NaCl B) H2O C) CO2 D) NH3
A) Transfer of electrons between atoms B) Sharing of electrons between atoms C) Presence of positive ions in a sea of delocalized electrons D) Formation of covalent bonds between atoms
A) Iron B) Carbon dioxide C) Sodium chloride D) Water
A) All of the above B) Electron affinity of atoms C) Electronegativity difference between atoms D) Atomic radius of atoms
A) Carbon B) Nitrogen C) Oxygen D) Helium
A) Strong electrostatic attractions between ions B) Weak intramolecular forces within molecules C) Weak intermolecular forces between molecules D) Strong covalent bonds between atoms
A) Methane (CH4) B) Hydrogen peroxide (H2O2) C) Sodium chloride (NaCl) D) Ethanol (C2H5OH)
A) Are closely packed together B) Have fixed positions in a lattice structure C) Have strong intermolecular forces of attraction D) Have negligible volume compared to the space they occupy
A) The chemical reactions occurring within a gas B) The density of particles within a gas C) The arrangement of particles within a gas D) The motion of particles within a gas
A) Digestion of food B) Burning of wood C) Rusting of iron D) Melting of ice
A) Pressure and volume of a gas B) Volume and number of moles of a gas C) Temperature and volume of a gas D) Pressure and temperature of a gas
A) PV = nT B) P = V/nRT C) PV = nRT D) PV = RT
A) Temperature B) Volume C) Square root of its molar mass D) Pressure
A) Atomic mass B) Volume C) Density D) Number of moles
A) Electrons in one atom of a substance B) Particles in one gram of a substance C) Moles in one liter of a gas D) Atoms in one mole of a substance
A) HCN B) CO2 C) H2O D) NH3
A) Both elements are non-metals B) Large difference in electronegativity C) High similarity in electronegativity D) Similar electron affinity values
A) Chlorine B) Sodium C) Helium D) Oxygen
A) They can be polar or non-polar B) They are responsible for the high melting and boiling points of many molecules. C) They involve sharing electrons. D) They form between atoms with similar electronegativity.
A) Dipole-dipole interactions B) London dispersion forces C) Hydrogen bonding D) Covalent bonding
A) They occupy a significant volume. B) They have specific shapes. C) They attract each other strongly D) They are constantly in motion.
A) solids are rigid and have definite shapes B) liquids flow easily and have indefinite shapes. C) gases expand to fill their container. D) all three statements are true.
A) dependent on the container size. B) directly proportional to its temperature C) inversely proportional to its temperature D) constant
A) R B) V C) P D) K
A) wood decreases, while the mass of the products remains constant. B) wood and oxygen is greater than the mass of the products. C) wood and oxygen is less than the mass of the products. D) wood and oxygen is equal to the mass of the carbon dioxide and water vapor.
A) reactants and products are used to convert between grams and moles. B) elements are used directly. C) are not needed, only the coefficients are important. D) compounds are ignored.
A) balance the chemical equation first. B) memorize the names of all elements and compounds. C) perform complex mathematical calculations. D) know the physical properties of all the reactants and products.
A) Water (H₂O) always contains hydrogen and oxygen in a 2:1 ratio by mass. B) The color of a compound can vary depending on its source. C) Carbon dioxide (CO₂) has a constant ratio of carbon to oxygen, regardless of its origin. D) All samples of table salt (NaCl) have the same ratio of sodium to chlorine.
A) 1:2 B) Cannot be determined without additional information. C) 2:3 D) 1:3/2
A) 2 grams of hydrogen react with 1 gram of oxygen to produce water. B) Two molecules of hydrogen react with one molecule of oxygen to form two molecules of water. C) Hydrogen and oxygen react explosively to form water. D) Water can decompose into hydrogen and oxygen under specific conditions.
A) only elements, not compounds. B) all chemical reactions. C) compounds that can react with each other. D) elements that can form more than one compound with another element.
A) the relative amounts of each molecule or atom involved in the reaction. B) the order in which the reactants combine. C) the names of the reactants and products D) the states of matter of the reactants and products.
A) Cannot be determined without additional information. B) 2.5 moles C) 5 moles D) 10 moles |