Chemistry Chapter 5 Questions

What group of elements is located on the very left of the periodic table? a) Alkali metals b) Alkaline earth metals c) Noble gases d) Halogens e) Metalloids

a) Alkali metals

Which of the following properties were NOT used to help Mendeleev develop the early periodic table of elements? a) Atomic number b) Density c) Atomic mass d) How the element formed a compound with hydrogen or oxygen e) Patterns of properties

a) Atomic number

Calculate the number of electrons the following ion has lost or gained: P3-? a) Gained 3 electrons b) Gained 3 protons c) Gained 1 electron d) Lost 3 electrons e) Lost 1 electron

a) Gained 3 electrons

Which of the following choices contains ONLY naturally occurring diatomic molecules? a) Nitrogen, bromine, and hydrogen b) Fluorine, oxygen, and sulfur c) Bromine, oxygen, and carbon d) Chlorine, bromine, and phosphorus e) Nitrogen, oxygen, and carbon

a) Nitrogen, bromine, and hydrogen

Covalent bonds tend to form with which families on the periodic table? a) Non-metals with other non-metals b) Halogens with noble gases c) Non-metals with noble gases d) Metals with non-metals e) Metals with other metals

a) Non-metals with other non-metals

Name the following compound: KNO3. a) Potassium nitrate b) Potassium nitrite c) Kadium nitrite d) Potassium nitrate oxygen e) Kadium nitrate

a) Potassium nitrate

Identify the following as compounds, molecules, or both: H2 (hydrogen) and CaS (calcium sulfide). a) H2 is a compound and CaS is both b) H2 is a molecule and CaS is a compound c) Both are molecules d) Both are compounds e) H2 is a molecule and CaS is both

b) H2 is a molecule and CaS is a compound

Which of the following families is considered to be the least reactive on the periodic table? a) Metalloids b) Noble gases c) Transition metals d) Halogens e) Alkali metals

b) Noble gases

Which of the following characteristics describes an ionic substance? a) Does not dissolve well in water b) Solid at room temperature c) Low bond strength d) Does not conduct electricity e) Low melting points

b) Solid at room temperature

What is typically the charge of chlorine, Cl, when it is an ion? a) 2- b) 1+ c) 1- d) 2+ e) Neutral

c) 1-

What is a polyatomic ion? a) A molecule that does not occur as a single element naturally b) A small molecule that does not make a difference in a reaction c) A small molecule with an overall positive or negative charge d) A molecule that only contains one element e) A molecule that breaks apart when dissolving

c) A small molecule with an overall positive or negative charge

Which of the following polyatomic ions would exhibit a positive charge? a) SO4?, sulfate b) OH?, hydroxide c) NH4?, ammonium d) C2H3O2?, acetate e) NO3?, nitrate

c) NH4?, ammonium

What is special about the way period numbers and group numbers work for lanthanide and actinide elements on the periodic table? a) Group numbers are not special, but period numbers are unique because lanthanides and actinides have negative period numbers b) Period numbers are not special, but group numbers are unique because lanthanides and actinides don't have group numbers c) Period numbers are not special, but group numbers are unique because lanthanides and actinides share the same group number d) Group numbers are not special, but period numbers are unique because lanthanides and actinides share the same period number e) Group numbers and period numbers are equal to each other only for these elements

c) Period numbers are not special, but group numbers are unique because lanthanides and actinides share the same group number

Which of the following options describe ONLY ionic compounds? a) Gas at room temperature, conducts electricity in liquid state, and high melting and boiling points b) Solid at room temperature, does not conduct electricity in solid state, and low melting and boiling points c) Solid at room temperature, does not conduct electricity in solid state, and high melting and boiling points d) Gas at room temperature, does not conduct electricity in liquid state, and high melting and boiling points e) Solid at room temperature, does not conduct electricity in liquid state, and high melting and boiling points

c) Solid at room temperature, does not conduct electricity in solid state, and high melting and boiling points

What is the formula for calcium phosphate? a) Ca(PO)4 b) Ca3PO2 c) Ca3P2 d) Ca3(PO4)2 e) Ca2(PO3)3

d) Ca3(PO4)2

What group of elements is found in the column prior to the last column on the periodic table? a) Noble gases b) Alkaline earth metals c) Alkali metals d) Halogens e) Transition metals

d) Halogens

What type of chemical bond does the following describe? A chlorine atom gains an electron becoming negative and a lithium atom loses an electron and becomes positive. The positives and negatives are attracted to each other and form bonds that are not localized to a single pair of atoms. a) Covalent bond b) A combination of an ionic and covalent bond c) Electronic bond d) Ionic bond e) Metallic bond

d) Ionic bond

Name the compound NaHCO3. a) Sodium carbonite b) Sodium carbonate c) Sodium acetate d) Sodium bicarbonate e) Sodium chlorate

d) Sodium bicarbonate

What is the difference between naming binary compounds compared to naming compounds that contain polyatomic ions? a) The rule of the metal cations using the element name is not applicable when naming compounds that contain polyatomic ions. b) There is no difference, both methods follow the same set of rules with no distinct differences. c) The cations must get the ending of "-ide" when naming compounds that contain polyatomic ions. d) The rule of the anion getting the "-ide" suffix is not applicable when naming compounds that contain polyatomic anions. e) The anion name goes first when naming compounds that contain polyatomic ions.

d) The rule of the anion getting the "-ide" suffix is not applicable when naming compounds that contain polyatomic anions.

Which of the following must be true of an electrically neutral ionic crystal structure? a) The melting point must be low. b) The crystal is in the liquid state at room temperature. c) The ionic crystal must be able to conduct electricity in a solid, liquid, and gas state. d) The total positive charge of positive ions must be canceled out by the total negative charge from negative ions. e) The ratio of positive ions to negative ions must always be one-to-one, or reduce to one-to-one.

d) The total positive charge of positive ions must be canceled out by the total negative charge from negative ions.

Write the chemical formula for barium nitride. a) Ba2N3 b) BaN c) BaN2 d) Ba3NO2 e) Ba3N2

e) Ba3N2

What is the correct formula for mercury(I) chloride? a) MgCl2 b) HgCl2 c) MnCl2 d) AgCl e) Hg2Cl2

e) Hg2Cl2

What group is on the very right of the periodic table? a) Halogens b) Alkaline earth metals c) Metalloids d) Alkali metals e) Noble gases

e) Noble gases

Why are parentheses used occasionally to write ionic chemical formulas? a) They act as an area for additional information such as ion charge of the atoms inside the parentheses. b) They groups the atoms inside the parentheses together to avoid confusion with neutral particles. c) They are used to make a distinguished separation between atoms in a chemical formula. d) They can be ignored because they have no significance. e) They maintain the correct ratio of atoms in a polyatomic ion when more than one ion is present.

e) They maintain the correct ratio of atoms in a polyatomic ion when more than one ion is present.

How many electrons are present in each ion respectively? a) Al3+; b) Ca2+; c) Cl-; d) Xe; e) Hg2+. a) a) 14e-; b) 20e-; c) 18e-; d) 77e-; e) 120e- b) a) 16e-; b) 22e-; c) 16e-; d) 54e-; e) 84e- c) a) 17e-; b) 22e-; c) 17e-; d) 77e-; e) 124e- d) a) 13e-; b) 20e-; c) 17e-; d) 54e-; e) 80e- e) a) 10e-; b) 18e-; c) 18e-; d) 54e-; e) 78e-

e) a) 10e-; b) 18e-; c) 18e-; d) 54e-; e) 78e-