Reference no: EM13793077

Module 1

1.) What is the volume of 60.0 g of ether if the density of ether is 0.70 g/mL?

2.) What is the density of 50.0 mL of a substance that has a mass of 25 g?

3.) List each as being a physical change or a chemical change: butter melting, butter burning, sugar dissolving in water, a sandwich getting digested.

4.) List each as being a physical or a chemical property: copper sulfate is blue, iron is a solid, water melts at 0^oC, gasoline is flammable, magnesium reacts with acid, salt is soluble in water.

5.) Correctly match the terms listed on the left with the substances listed on the right. More than one term may be used for each substance.

A. element                                 Mg

B. compound                             Fe mixed with sand

C. heterogeneous                       saltwater

D. mixture                                  water

E. homogeneous                         MgSO₄

F. pure substance

G. Solution

Module 2

1.) All atoms of the same element have the same number of _______.

2.) An atom of an element with atomic number 48 and mass number 120 contains ____ protons, ____ electrons, and ______ neutrons.

3.) What is the atomic number and the mass number of an atom of an element with 11 protons and 12 neutrons?

4.)  Cl     and       Cl are _______ of  each other. The first one has ______ protons and _____neutrons. The second one has ______ protons and _____neutrons.

Module 3

1.) What is the number of electrons in the outermost occupied energy level of an element in Group 5A?

2.) The electron configuration of calcium is _______.

3.) Why are the noble gases so unreactive?

4.) If the electron configuration of an element is 1s² 2s² 2p⁶ 3s² 3p⁵, the element is ______.

5.) Tell whether each of the following elements is an inner transition metal, noble gas, alkali metal, alkaline earth metal, or halogen. Then give its period and group numbers.

 a. calcium    b. cesium    c. fluorine    d. chromium    e. neon     f. silver

6.) A column of elements in the periodic table is known as a ________.

7.) Identify the following elements:

a. period 5 alkali metal.      b. period 4 halogen.     c. period 5 halogen.      d. period 5, Group IB.

Module 4

1.) The chemical formula for the ionic compound formed when elements of Ca and N react is ______, when lithium and sulfide ion react is ______, when iron (II) and chlorine react is ______, when aluminum and sulfate ion react is _______.

2.) Write the formulas and charges for the following ions: Phosphate, nitrite, nitrate, hydroxide, carbonate, ammonium.

3.) What is the total number of atoms in one molecule of C₆H_l2O₆?

4.) What types of elements when combined would be most likely to form an ionic compound?

5.) What is the ionic charge on the chromium ion in the ionic compound that has the formula Cr₂O₃?

6.) In a polyatomic ion the -ite ending indicates one fewer  _______ atom than the -ate ending.

7.) The ionic charge of lead, Pb, in the compound PbS₂ is _________.

8.) If a bonding pair of electrons is unequally shared between two atoms, the bond is ______. What are some properties of polar compounds compared to nonpolar compounds?

9.) Which elements exist as diatomic molecules?

Module 5

1.) How many formula units are in 1 mole of (NH₄)₂SO₄?

2.) How many moles are in 8.5 x 10²⁶ molecules of CO₂?

3.) How many grams are in 6.51 moles of H₂SO₄?

4.) How many moles are in 2.56 x 10^-4 grams of Fe₂O₃?

Module 6

1.) Identify the type of reaction for those listed below:

A. a reaction in which a single compound is broken down into simpler substances

B. a reaction in which oxygen reacts with another substance, often producing heat or light

C. a reaction in which the atoms of one element replace the atoms of a cation in a compound

D. a reaction in which two or more substances react to form a single substance

E. a reaction that involves an exchange of positive ions between two compounds

2.) A double-replacement reaction takes place when aqueous K₂SO₄ reacts with aqueous Pb(NO₃)₂. You would

        expect the products of this reaction to be ______ and _____.

3.) The equation H₃PO₄ + 3KOH → K₃PO₄ + 3H₂O is an example of which reaction?

4.) Balance the following equations and state the type of reaction:

          A. Ca(s) + H₃PO₄(aq) → Ca₃(PO₄)₂ (s) + H₂(g)

          B. KBrO₃(s) → KBr(s) + O₂(g)

Module 7

1.) Refer to the following equation:

3Cu(s) + 8HNO₃(aq) → 3Cu(NO₃)₂(s) + 2NO(g) + 4H₂O(l)

 

A. 6 moles of Cu will produce _____ moles of H₂O.

B. Calculate the number of moles of water produced when 3.3 mol of Cu(NO₃)₂ are formed in the reaction.

C. How many grams of Cu would be needed to react with 2.0 mol HNO₃?

D. If you could drop 12 atoms of copper into a beaker containing nitric acid, how many molecules of NO would

     be produced?

E. If you have 8 atoms of nitrogen on the reactant side of the equation, then how many atoms of nitrogen will be

    on the product side of the equation?

F. How many grams of NO would be made from 16 grams of Cu in the reaction.