Default Title

Question (1)

QN0035972

Carbon has atomic number 6. Which electronic configuration explains its ability to form covalent bonds rather than readily forming C⁴⁺ or C⁴⁻ ions?

(A) 2,4
(B) 2,6
(C) 4,2
(D) 6,0

Correct Answer: A

Explanation:

Carbon has four electrons in its outermost shell. Losing or gaining four electrons is energetically difficult, so it shares electrons to form covalent bonds.

Link:

Report Error

Question (2)

QN0035973

A carbon atom shares one electron with each of four hydrogen atoms. How many shared electron pairs are present in the resulting methane molecule?

(A) 2
(B) 3
(C) 4
(D) 5

Correct Answer: C

Explanation:

Carbon forms four single covalent bonds with four hydrogen atoms in CH₄. Each single bond represents one shared electron pair.

Link:

Report Error

Question (3)

QN0035974

Which observation would most strongly indicate that a compound has covalent bonding rather than ionic bonding?

(A) It has a very high melting point and conducts in molten state.
(B) It contains ions in solution.
(C) It has low melting and boiling points and generally does not conduct electricity.
(D) It conducts electricity in the solid state.

Correct Answer: C

Explanation:

Most covalent carbon compounds have weak intermolecular forces, low melting/boiling points and are poor conductors because they do not produce ions.

Link:

Report Error

Question (4)

QN0035975

Oxygen has six valence electrons. When two oxygen atoms form O₂, how many pairs of electrons are shared between them?

(A) One
(B) Two
(C) Three
(D) Four

Correct Answer: B

Explanation:

Each oxygen atom needs two more electrons, so the atoms share two pairs, forming a double bond.

Link:

Report Error

Question (5)

QN0035976

Nitrogen has five valence electrons. If two nitrogen atoms form N₂, how many covalent bonds are required to complete the octet of both atoms?

(A) One
(B) Two
(C) Three
(D) Four

Correct Answer: C

Explanation:

Each nitrogen atom contributes three electrons for sharing, producing three shared pairs—a triple bond.

Link:

Report Error

Question (6)

QN0035977

A student compares diamond and graphite, both made only of carbon. Which structural difference best explains their different physical properties?

(A) Diamond contains carbon while graphite contains oxygen.
(B) Diamond has a three-dimensional network, while graphite has layered structures.
(C) Diamond is ionic while graphite is covalent.
(D) Diamond contains hydrogen while graphite does not.

Correct Answer: B

Explanation:

In diamond each carbon is bonded to four other carbon atoms in a rigid 3-D structure, while graphite has carbon atoms arranged in layers.

Link:

Report Error

Question (7)

QN0035978

Graphite can conduct electricity even though carbon is a non-metal. Which structural feature helps explain this?

(A) It contains metal ions.
(B) It has a layered structure with carbon atoms bonded in planes.
(C) It contains water molecules.
(D) It has no covalent bonds.

Correct Answer: B

Explanation:

Graphite has a different bonding arrangement from diamond and is specifically noted in the chapter as a good conductor of electricity.

Link:

Report Error

Question (8)

QN0035979

A carbon compound contains only single bonds between carbon atoms. Which classification is most appropriate?

(A) Unsaturated
(B) Saturated
(C) Aromatic only
(D) Ionic

Correct Answer: B

Explanation:

Carbon compounds containing only single bonds between carbon atoms are saturated compounds.

Link:

Report Error

Question (9)

QN0035980

A compound contains a carbon-carbon double bond. If all other features are consistent with the chapter's classification, which statement is correct?

(A) It is necessarily an alkane.
(B) It is an unsaturated compound.
(C) It must be an alcohol.
(D) It must contain no hydrogen.

Correct Answer: B

Explanation:

Compounds containing double or triple bonds between carbon atoms are classified as unsaturated compounds.

Link:

Report Error

Question (10)

QN0035981

Why can carbon form millions of compounds even though it has only four valence electrons?

(A) It forms only ionic bonds.
(B) It has tetravalency and strong carbon-carbon bonding.
(C) It has no valence electrons.
(D) It can form only short chains.

Correct Answer: B

Explanation:

Carbon's tetravalency allows bonding with four atoms, while catenation allows carbon atoms to form stable chains, branches and rings.

Link:

Report Error

Question (1)

Carbon has atomic number 6. Which electronic configuration explains its ability to form covalent bonds rather than readily forming C⁴⁺ or C⁴⁻ ions?

Explanation:

Link:

Question (2)

A carbon atom shares one electron with each of four hydrogen atoms. How many shared electron pairs are present in the resulting methane molecule?

Explanation:

Link:

Question (3)

Which observation would most strongly indicate that a compound has covalent bonding rather than ionic bonding?

Explanation:

Link:

Question (4)

Oxygen has six valence electrons. When two oxygen atoms form O₂, how many pairs of electrons are shared between them?

Explanation:

Link:

Question (5)

Nitrogen has five valence electrons. If two nitrogen atoms form N₂, how many covalent bonds are required to complete the octet of both atoms?

Explanation:

Link:

Question (6)

A student compares diamond and graphite, both made only of carbon. Which structural difference best explains their different physical properties?

Explanation:

Link:

Question (7)

Graphite can conduct electricity even though carbon is a non-metal. Which structural feature helps explain this?

Explanation:

Link:

Question (8)

A carbon compound contains only single bonds between carbon atoms. Which classification is most appropriate?

Explanation:

Link:

Question (9)

A compound contains a carbon-carbon double bond. If all other features are consistent with the chapter's classification, which statement is correct?

Explanation:

Link:

Question (10)

Why can carbon form millions of compounds even though it has only four valence electrons?

Explanation:

Link:

Excel With Tutors

ExcelWithTutors

For Student

For Tutors

Learn

OUR POLICY