Deck 10: The Periodic Law

Question 1

A vertical column in the periodic table is called a

A) shell.
B) subshell.
C) group.
D) period.

Answer 1

group.

Question 2

Which of the following is a heterogeneous mixture?

A) seawater
B) salt
C) soil
D) gasoline

Answer 2

soil

Question 3

The statement that the elements in a given compound are always combined in the same proportions by mass is known as

A) the periodic law.
B) the law of definite proportions.
C) the law of conservation of mass.
D) Dalton's law.

Answer 3

the law of definite proportions.

Question 4

The least active of the following nonmetals is

A) oxygen.
B) fluorine.
C) sulfur.
D) helium.

Question 5

The most active of the following nonmetals is

A) oxygen.
B) fluorine.
C) sulfur.
D) helium.

Question 6

Which of the following statements is not true of all metals?

A) They conduct heat well.
B) They conduct electric current well.
C) They are solids at room temperature.
D) They are opaque to light.

Question 7

The atomic mass of an element is

A) the average atomic mass of its isotopes according to their proportions in nature.
B) the average mass number of its isotopes according to their proportions in nature.
C) the average atomic number of its isotopes according to their proportions in nature.
D) the atomic mass of its most abundant isotope.

Question 8

The most abundant element in the universe is

A) hydrogen.
B) helium.
C) oxygen.
D) carbon.

Question 9

The least active of the following metals is

A) silver.
B) potassium.
C) zinc.
D) copper.

Question 10

Known elements have atomic numbers up to

A) 92
B) 100
C) 118
D) 150

Question 11

The largest number of elements are classed as

A) metals.
B) inert gases.
C) nonmetals.
D) liquids.

Question 12

Carbon

A) is a typical metal.
B) is a typical nonmetal.
C) has properties intermediate between those of metals and nonmetals.
D) has properties no other element has.

Question 13

At room temperature, bromine is a

A) colorless gas.
B) greenish-yellow gas.
C) reddish-brown liquid.
D) steel-gray solid.

Question 14

According to the periodic table, the chemical properties of the elements are periodic functions of their

A) density.
B) atomic number.
C) atomic mass.
D) mass number.

Question 15

Which of the following is a homogeneous mixture?

A) blood
B) air
C) water
D) sugar

Question 16

The scientist who first established the relative masses of different elements was

A) Mendeleev.
B) Maxwell.
C) Priestley.
D) Dalton.

Question 17

The metals most difficult to extract from their ores in general

A) are the least active chemically.
B) are the most active chemically.
C) have the lowest atomic numbers.
D) have the highest atomic numbers.

Question 18

Which of the following is a compound?

A) ice
B) granite
C) helium
D) milk

Question 19

Of the halogens, at room temperature and atmospheric pressure

A) all are gases.
B) one is a gas and the others are liquids.
C) one is a gas and the others are solids.
D) one is a liquid and the others are gases or solids.

Question 20

The most active of the following metals is

A) silver.
B) potassium.
C) zinc.
D) copper.

Question 21

An atom whose outer electron shell lacks one electron from being filled is

A) a halogen.
B) an active metal.
C) an inactive metal.
D) an inert gas.

Question 22

A bonding molecular orbital

A) always consists of s atomic orbitals that overlap.
B) always consists of p atomic orbitals that overlap.
C) always consists of one s and one p atomic orbital that overlap.
D) may consist of any of the above overlaps.

Question 23

An element that can form an ionic compound with oxygen is

A) carbon.
B) calcium.
C) nitrogen.
D) neon.

Question 24

A family of elements whose atoms react by picking up electrons is the

A) alkali metals.
B) halogens.
C) transition metals.
D) inert gases.

Question 25

Each horizontal row of the periodic table includes elements with chemical characteristics that are, in general,

A) identical.
B) similar.
C) different.
D) sometimes similar and sometimes different.

Question 26

The rare earth elements are not

A) extremely rare in the earth's crust.
B) found in ores in the United States.
C) used in exceptionally strong magnets.
D) used in certain lasers and other light sources.

Question 27

Ionic compounds in the solid state

A) always consist of molecules.
B) sometimes consist of molecules.
C) never consist of molecules.
D) never occur as crystals.

Question 28

Organic compounds

A) are covalent and contain carbon.
B) are covalent and may contain carbon.
C) contain carbon and may be covalent.
D) may contain carbon and may be covalent.

Question 29

Each electron shell in an atom contains

A) the same number of electrons as all its other shells.
B) electrons whose energies are exactly the same.
C) electrons with the same principal quantum number n.
D) electrons with the same probability clouds.

Question 30

Table salt, NaCl, consists of

A) molecules of Na and Cl with covalent bonds between their atoms.
B) molecules of Na and Cl with ionic bonds between their ions.
C) crystals of Na and Cl with covalent bonds between their atoms.
D) crystals of Na and Cl with ionic bonds between their ions.

Question 31

A free radical is extremely reactive because it

A) is a negative ion.
B) is a positive ion.
C) contains an unpaired electron.
D) contains only paired electrons.

Question 32

The inert gases

A) have the same atomic number.
B) are in the same period of the periodic table.
C) are in the same group of the periodic table.
D) join in pairs to form diatomic molecules.

Question 33

A molecule that does not contain a polar covalent bond is

A) CO.
B) BrF.
C) HI.
D) Cl₂.

Question 34

An atom whose outer electron shell is filled is

A) a halogen.
B) an active metal.
C) an inactive metal.
D) an inert gas.

Question 35

Elements with similar properties other than atomic mass)

A) occupy the same period of the periodic table.
B) have similar electron configurations.
C) have the same number of neutrons in their nuclei.
D) exist in the same physical state solid, liquid, or gas).

Question 36

Atoms of two different elements

A) may form no compounds together.
B) can form only one compound together.
C) can always form more than one compound together.
D) must form ions of the same charge if they are to form a compound together.

Question 37

When atoms join to form a molecule,

A) energy is absorbed.
B) energy is given off.
C) energy is neither absorbed nor given off.
D) Any of these choices, depending on the circumstances.

Question 38

The elements with the highest ionization energies are the

A) alkali metals
B) halogens
C) inert gases
D) rare earths

Question 39

In a covalent compound

A) electrons are shifted from one atom to another.
B) only atoms of the same element are present.
C) there must be at least one carbon atom.
D) adjacent atoms share electron pairs.

Question 40

A horizontal row in the periodic table is called a

A) shell.
B) subshell.
C) group.
D) period.

Question 41

The missing number in the equation 6H₃BO₃ → H₄B₆O₁₁ + )H₂O is

A) 1.
B) 6.
C) 7.
D) 14.

Question 42

The ion of the hydroxide group has the symbol

A) OH.
B) OH⁺.
C) OH^-.
D) H₂O^-.

Question 43

The number of compounds that carbon and oxygen can form is

A) 1.
B) 2.
C) 3.
D) 4.

Question 44

The number of oxygen atoms in a molecule of aluminum sulfate, Al₂SO₄)₃, is

A) 3.
B) 4.
C) 7.
D) 12.

Question 45

The charge on halogen ions is

A) +1.
B) +2.
C) -1.
D) -2.

Question 46

The missing number in the equation 4NH₃ + [ ]O₂ → 4NO + 6H₂O is

A) 1.
B) 2.
C) 5.
D) 10.

Question 47

The number of atoms in a molecule of ammonium sulfide, NH₄)₂S, is

A) 3.
B) 6.
C) 10.
D) 11.

Question 48

The electrolysis of water is an example of a

A) combination reaction.
B) decomposition reaction.
C) single displacement reaction.
D) double displacement reaction.

Question 49

The number of H₂O molecules needed to react with 1 atom of Be to form H₂ and BaOH)₂ is

A) 1.
B) 2.
C) 4.
D) 8.

Question 50

A compound whose name ends in -ate always contains

A) hydrogen.
B) oxygen.
C) one or more hydroxide groups.
D) only two elements.

Question 51

The name of the compound Ca₃N₂ is

A) calcium nitride.
B) calcium nitrate.
C) calcium nitrite.
D) calcium trinitride.

Question 52

Potassium forms K⁺ ions and sulfur forms S^2- ions. The formula of potassium sulfide is

A) KS.
B) K₂S.
C) KS₂.
D) K₂S₂.

Question 53

The missing number in the equation 2CaNO₃)₂ → 2CaO + [ ]NO₂ + O₂ is

A) 1.
B) 2.
C) 3.
D) 4.

Question 54

The chromate ion has the formula CrO₄^2-. The formula of tinI) chromate is

A) SnCrO₄.
B) Sn₂CrO₄.
C) SnCrO₄)₂.
D) Sn₂CrO₄)₂.

Question 55

The number of units of NaOH needed to react with 1 unit of H₃PO₄ to form Na₃PO₄ and H₂O is

A) 1.
B) 2.
C) 3.
D) 4.

Question 56

Which of the following chemical equations is balanced?

A) Fe₂O₃ + CO → Fe + 2CO₂
B) Na₂SO₂ + S → S₂O₃ + S
C) 3CuO + 2NH₃ → 3Cu + 3H₂O + N₂
D) 4Al + 3Fe₃O₄ → 4Al₂O₃ + 9Fe

Question 57

AgNO₃ reacts with CaCl₂ to form AgCl and CuNO₃)₂. The number of units of AgNO₃ needed to form one unit of CuNO₃)₂ in this reaction is

A) 1.
B) 2.
C) 3.
D) 4.

Question 58

The charge on alkali metal ions is

A) +1.
B) +2.
C) -1.
D) -2.

Question 59

The nitrate ion has the formula NO₃^-. The formula of mercuryII) nitrate is

A) HgNO₃.
B) Hg₂NO₃.
C) HgNO₃)₂.
D) Hg₂NO₃)₂.