WorksheetsReview 5,6
Total questions: 41
Worksheet time: 21mins
The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed to
Mendeleev.
Moseley.
Bohr.
Ramsay.
The person whose work led to a periodic table based on increasing atomic number was
Moseley.
Mendeleev.
Rutherford.
Cannizzaro.
The discovery of what elements added a new column to Mendeleev's periodic table?
noble gases
radioactive elements
transition elements
metalloids
The periodic law allows some properties of an element to be predicted based on its
position in the periodic table.
number of isotopes.
symbol.
color.
A horizontal row of blocks in the periodic table is called a(n)
group.
period.
family.
octet.
How many elements are in a period in which only the s and p sublevels are filled?
2
8
18
32
The electron configuration of an element is [Kr] 4d6 5s1. To what group does this element belong?
Group 4
Group 5
Group 7
Group 9
Which block in the periodic table contains the alkali metals?
s
p
d
f
The most characteristic property of the noble gases is that they
have low boiling points.
are radioactive.
are gases at ordinary temperatures.
are largely unreactive.
When determining the size of an atom by measuring the distance between bonded, identical, adjacent nuclei, the radius of an atom is
equal to the distance between nuclei.
one-half the distance between nuclei.
twice the distance between nuclei.
one-fourth the distance between nuclei.
Which represents a neutral atom acquiring an electron in a process where energy is released?
A + e- + energy → A-
A + e- → A- + energy
The energy required to remove an electron from an atom is the atom's
electron affinity.
electron energy.
electronegativity.
ionization energy.
The element that has the greatest electronegativity is
oxygen.
sodium.
chlorine.
fluorine.
A positive ion is known as a(n)
ionic radius.
valence electron.
cation.
anion.
A negative ion is known as a(n)
ionic radius.
valence electron.
cation.
anion.
In a row in the periodic table, as the atomic number increases, the atomic radius generally
decreases.
remains constant.
increases.
becomes immeasurable.
Within a group of elements, as the atomic number increases, the atomic radius
increases.
remains approximately constant.
decreases regularly.
varies unpredictably.
The ionization energies for removing successive electrons from sodium are 496 kJ/mol, 4562 kJ/mol, 6912 kJ/mol, and 9544 kJ/mol. The great jump in ionization energy after the first electron is removed indicates that
sodium has four or five electrons.
the atomic radius has increased.
a d electron has been removed.
the noble gas configuration has been reached.
The ionization energies required to remove successive electrons from one mole of calcium atoms are 590 kJ/mol, 1145 kJ/mol, 4912 kJ/mol, and 6474 kJ/mol. The most common ion of calcium is probably
Ca+.
Ca2+.
Ca3+.
Ca4+.
The force of attraction by Group 1 metals for their valence electrons is
weak.
zero.
strong.
greater than that for inner shell electrons.
The electrons available to be lost, gained, or shared when atoms form compounds are called
ions.
valence electrons.
d electrons.
electron clouds.
A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together is called a(n)
ion.
molecule.
chemical bond.
electron cloud.
Atoms naturally move
toward high potential energy.
toward low potential energy.
toward less stability.
away from each other.
If two covalently bonded atoms are identical, the bond is
nonpolar covalent.
polar covalent.
dipole covalent.
coordinate covalent.
If the atoms that share electrons have an unequal attraction for the electrons, the bond is called
nonpolar.
polar.
ionic.
dipolar.
The greater the electronegativity difference between two bonded atoms, the greater the percentage of ____ in the bond.
ionic character
covalent character
metallic character
electron sharing
The B—F bond in BF₃ (electronegativity for B is 2.0; electronegativity for F is 4.0) is
polar covalent.
ionic.
nonpolar covalent.
metallic.
In the three molecules, O₂, HCl, and F₂, what atom would have a partial negative charge?
oxygen
hydrogen
chlorine
fluorine
The electron configuration of nitrogen is 1s² 2s² 2p³. How many more electrons does nitrogen need to satisfy the octet rule?
1
3
5
8
In drawing a Lewis structure, the central atom is generally the
atom with the greatest mass.
atom with the highest atomic number.
atom with the fewest electrons.
least electronegative atom.
The substance whose Lewis structure shows three covalent bonds is
H₂O.
CH₂Cl₂.
NH₃.
CCl₄.
What is the correct Lewis structure for hydrogen chloride, HCl?
Cl — H:
:H — Cl:
:H — Cl::
H — Cl:::
The ions in most ionic compounds are organized into a
molecule.
Lewis structure.
polyatomic ion.
crystal.
If the lattice energy of compound A is greater than that of compound B,
compound A is not an ionic compound.
the bonds in compound A are stronger than the bonds in compound B.
compound B is probably a gas.
compound A has larger crystals than compound B.
How many extra electrons are in the Lewis structure of the phosphate ion, PO43− ?
0
2
3
4
The mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals of equal energies is called
VSEPR theory.
malleability.
hybridization.
dipole-dipole interaction.
42. Select the correct Lewis structure for carbon disulfide, CS2.
S=C=S with double bonds between C and each S, no lone pairs on C, four lone pairs on each S
S-C-S with single bonds between C and each S, two lone pairs on each S and C
S=C=S with single bonds between C and each S, two lone pairs on each S and C
S-C≡S with a triple bond between C and one S, single bond to the other S, lone pairs distributed
Analyze ionic and covalent compounds in terms of their formation (electron transfer vs. sharing), names, chemical formulas.
Ionic compounds form by electron transfer, covalent by electron sharing; both have distinct naming rules and chemical formulas.
Ionic and covalent compounds both form by electron sharing and have identical naming rules.
Ionic compounds form by electron sharing, covalent by electron transfer; both have the same chemical formulas.
Ionic and covalent compounds have no differences in formation, naming, or formulas.
Covalent and ionic compounds differ in their bonding and properties. Which statement best compares and contrasts covalent and ionic compounds?
Covalent compounds share electrons, while ionic compounds transfer electrons; covalent compounds tend to have lower melting points than ionic compounds.
Covalent compounds transfer electrons, while ionic compounds share electrons; both have high melting points.
Both covalent and ionic compounds share electrons and have similar melting points.
Ionic compounds have lower melting points than covalent compounds, and both transfer electrons.
How many valence electrons are present in a molecule with 2 carbon atoms and 4 oxygen atoms, with a charge of -2?
34 valence electrons. Calculation: (2 x 4) + (4 x 6) + 2 = 8 + 24 + 2 = 34.
30 valence electrons. Calculation: (2 x 4) + (4 x 6) = 8 + 24 = 32.
36 valence electrons. Calculation: (2 x 4) + (4 x 6) + 4 = 8 + 24 + 4 = 36.
32 valence electrons. Calculation: (2 x 4) + (4 x 6) = 8 + 24 = 32.
How many valence electrons are present in a molecule with 1 carbon atom and 2 sulfur atoms?
16 valence electrons. Calculation: (1 x 4) + (2 x 6) = 4 + 12 = 16.
12 valence electrons. Calculation: (1 x 4) + (2 x 4) = 4 + 8 = 12.
18 valence electrons. Calculation: (1 x 6) + (2 x 6) = 6 + 12 = 18.
20 valence electrons. Calculation: (1 x 4) + (2 x 8) = 4 + 16 = 20.
