1 Bilal is writing the molecular formula for glucose. He knows that the empirical formula is CH2O and the molar mass is 180 g/mol. What is the molecular formula? A C3H6O3 B C4H8O4 C C5H10O5 D C6H12O6
2 Fatima is writing the chemical formula for sodium oxide. Sodium has a +1 charge and oxide has a -2 charge. What is the formula? A NaO B Na2O C NaO2 D Na2O2
3 Which term is used for ionic compounds instead of molecular mass? A Atomic mass B Formula mass C Gram mass D Relative mass
4 Xia is learning about binary ionic compounds. She wants to write the formula for calcium fluoride. What is the correct formula? A CaF B CaF2 C Ca2F D CaF3
5 A balanced chemical equation follows the law of: A Constant proportion B Multiple proportion C Conservation of mass D Definite composition
6 Tina is calculating the mass of 0.25 moles of NaCl. The molar mass of NaCl is 58.5 g/mol. What is the mass? A 14.625 g B 29.25 g C 58.5 g D 7.3125 g
7 Molecular formula shows: A Simplest ratio of atoms B Percentage composition C Actual number of atoms D Ionic charge
9 Hina is studying gram atomic mass. She knows that the gram atomic mass of an element is the mass of one mole of atoms of that element. What is the gram atomic mass of oxygen? A 8 g B 16 g C 24 g D 32 g
10 Zara has 5 moles of NaCl. How many formula units of NaCl does she have? A 3.011 × 10^24 formula units B 6.022 × 10^23 formula units C 1.204 × 10^24 formula units D 1.806 × 10^24 formula units
11 Uma is learning about mole-particle calculations. She knows that the number of particles = moles × Avogadro's number. If she has 2.5 moles of CO2, how many molecules? A 1.506 × 10^24 molecules B 6.022 × 10^23 molecules C 1.204 × 10^24 molecules D 1.806 × 10^24 molecules
12 Fatima is learning about Avogadro's number. She knows that one mole of any substance contains 6.022 × 10^23 particles. What is this number called? A Avogadro's number B Plank's constant C Molar volume D Gas constant
13 Sam is calculating the number of particles in 2 moles of CO2. How many molecules of CO2 are present? A 1.204 × 10^24 molecules B 6.022 × 10^23 molecules C 3.011 × 10^23 molecules D 1.806 × 10^24 molecules
14 Patricia is exploring ionic equations. She writes the complete ionic equation for a reaction. What is the difference between a molecular equation and an ionic equation? A Ionic equation shows all ions, molecular equation shows complete compounds B Molecular equation shows all ions, ionic equation shows complete compounds C Both are identical D Ionic equation is for solids only
15 To convert moles into particles, we multiply by: A Atomic mass B Molecular mass C Avogadro’s number D Density
16 If empirical formula is CH2 and molecular mass is 28, molecular formula is: A CH2 B C2H4 C C3H6 D CH4
17 Empirical formula shows: A Actual number of atoms B Simplest whole number ratio C Total mass of compound D Structural arrangement
18 Lara is calculating the number of molecules in 0.5 moles of CO2. How many molecules? A 3.011 × 10^23 molecules B 6.022 × 10^23 molecules C 1.204 × 10^24 molecules D 1.806 × 10^24 molecules
19 Emma is naming binary ionic compounds. She has a compound formed from magnesium and chlorine. What is the correct name for this compound? A Magnesium chloride B Magnesium dichloride C Magnesium chlorate D Magnesium chlorite
20 Xia is writing the name for Fe2O3. She knows that iron can have multiple oxidation states. What is the correct name for Fe2O3? A Iron(II) oxide B Iron(III) oxide C Iron oxide D Ferric oxide
21 Oliver is calculating the number of moles in 36 g of water. The molar mass of water is 18 g/mol. How many moles? A 1 mole B 1.5 moles C 2 moles D 2.5 moles
23 Oliver is balancing a chemical equation. He has the equation: H2 + O2 → H2O. What is the coefficient of water when the equation is balanced? A 1 B 2 C 3 D 4
24 The substance left after reaction is called: A Limiting reagent B Excess reagent C Product D Catalyst