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Quizzes > Science

Ionic and Covalent Bonds Quiz: Test Bonding Basics

Quick chemistry quiz on ionic vs covalent bonds. Instant results and explanations.

Editorial: Review CompletedCreated By: Ahmed YasserUpdated Aug 24, 2025
Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
paper art chemistry icons represent ionic covalent bonds lewis dot structures octet rule quiz on coral background

This quiz helps you compare ionic and covalent bonds, apply the octet rule, and read Lewis dot structures in short questions. For more practice, try the ionic and covalent quiz, review a broader bond types quiz, and build skills with ionic formula practice before your next test.

What term describes an atom that has lost or gained electrons?
Molecule
Isotope
Radical
Ion
An ion is an atom or molecule that has gained or lost one or more electrons, resulting in a net electrical charge. Atoms form ions to achieve more stable electron configurations, often following the octet rule. Molecules, isotopes, and radicals have different definitions that do not specifically refer to charged species. .
In ionic bond formation, atoms achieve stability by transferring which subatomic particles?
Electrons
Photons
Protons
Neutrons
Ionic bonds form when one atom donates electrons to another, resulting in oppositely charged ions that attract each other. Neutrons and protons reside in the nucleus and are not transferred during bond formation. Photons are quanta of light and unrelated to bonding. .
Ionic compounds are typically formed between which types of elements?
Metalloid and gas
Two metals
Metal and nonmetal
Two nonmetals
Ionic compounds form when metals (which tend to lose electrons) react with nonmetals (which tend to gain electrons). Two metals cannot form ionic bonds since both prefer to lose electrons, and two nonmetals typically form covalent bonds. Metalloids and gases are not the common pairing for simple ionic salts. .
What structure is characteristic of solid ionic compounds?
Random network
Crystal lattice
Amorphous solid
Discrete molecules
Solid ionic compounds adopt a crystal lattice structure where ions are arranged in a repeating three-dimensional pattern. This maximizes attractive forces and minimizes repulsion. Discrete molecules or random networks are typical of covalent substances. .
When a sodium atom forms an ionic bond, it becomes a ...?
Isotope
Radical
Anion
Cation
Sodium loses one electron to achieve a stable electron configuration, resulting in a positively charged ion known as a cation. Anions are negatively charged and form when atoms gain electrons. Radicals and isotopes refer to different phenomena. .
Which term refers to positively charged ions?
Cations
Neutrals
Radicals
Anions
Cations are ions with a positive charge, formed when atoms lose electrons. Anions carry a negative charge after gaining electrons. Neutrals and radicals are not standard terms for positively charged species. .
Which rule states that atoms tend to gain, lose, or share electrons to obtain eight electrons in their valence shell?
Duet rule
Law of definite proportions
Hund's rule
Octet rule
The octet rule describes the tendency of atoms to achieve eight electrons in their valence shell, similar to the electron configuration of noble gases. The duet rule applies only to hydrogen and helium. The other laws govern different chemical principles. .
What is the charge on a chloride ion in an ionic compound such as NaCl?
+2
-1
+1
0
Chlorine gains one electron to form the chloride ion, resulting in a -1 charge. This completes its valence shell to resemble the noble gas argon. A +1 or +2 charge would indicate loss of electrons, not gain. .
Which of the following is the correct Lewis dot structure for a fluoride ion, F-?
F with six dots
F with eight dots and a negative sign
F with seven dots
F with no dots
The fluoride ion has gained one electron, giving it eight valence electrons represented by eight dots around the symbol F and a negative charge sign. Seven or six dots would not show a full valence shell, and no dots omits valence electrons entirely. .
What is the ionic charge on magnesium in the compound MgCl2?
-1
+2
-2
+1
In MgCl2 each chloride ion has a -1 charge and there are two chlorides, so magnesium must have a +2 charge to balance the overall neutrality. A +1 charge would not neutralize two chloride ions. .
Which of these compounds is ionic?
H2O
NaCl
CH4
CO2
NaCl is formed by the transfer of electrons between sodium and chlorine, making it ionic. CO2, H2O, and CH4 involve sharing of electrons between nonmetals and are covalent compounds. .
Why do ionic compounds generally have high melting points?
Hydrogen bonding
Metallic bonding
Weak van der Waals forces
Strong electrostatic forces between ions
Ionic compounds feature strong electrostatic attractions between oppositely charged ions that require significant energy to overcome. Weak van der Waals forces and hydrogen bonds are much weaker, and metallic bonding applies to metals, not ionic solids. .
How many electrons does an aluminum ion, Al3+, have?
13
16
12
10
Neutral aluminum has 13 electrons; when it forms Al3+ it loses three electrons, leaving it with 10 electrons. Losing three yields the +3 charge on the ion. .
Which of the following has the greatest ionic character based on electronegativity values: LiF, NaCl, KF, CsI?
NaCl
KF
CsI
LiF
LiF has the largest electronegativity difference between lithium and fluorine, leading to the highest ionic character. As the difference decreases in the other compounds, the bonds become less ionic. .
In the lattice energy trend of alkali halides, which factor leads to higher lattice energy?
Smaller ionic radii
Lower ionic charge
Larger ionic radii
Higher solubility
Lattice energy increases when ions are smaller because they can pack more closely, increasing electrostatic attraction. Larger ions and lower charges both reduce lattice energy. Solubility is unrelated to lattice energy. .
Which ion is larger in radius: Na+ or Mg2+ in the same period?
They are equal
Na+
Cannot compare
Mg2+
Both ions have the same number of electrons but Na+ has one less positive charge than Mg2+, so its electron cloud is less tightly held and thus larger. Mg2+ has a higher effective nuclear charge on the same number of electrons, pulling them closer. .
What is the oxidation state of phosphorus in the hexafluorophosphate ion, PF6^-?
+4
+3
+6
+5
In PF6^- each fluorine has a -1 charge (total -6), and the overall ion has a -1 charge, so phosphorus must be +5 to balance: x + (-6) = -1. Therefore, oxidation state of P is +5. .
Among the following compounds, which has the highest lattice energy: MgO, NaF, CaO, KCl?
KCl
CaO
MgO
NaF
MgO has the highest lattice energy due to the +2 and -2 charges on Mg2+ and O2- and their relatively small ionic radii, leading to very strong electrostatic attraction. The other salts have lower charges or larger ions, resulting in lower lattice energies. .
In the Born-Haber cycle, which step represents the energy required to remove an electron from a gaseous atom?
Sublimation energy
Electron affinity
Ionization energy
Enthalpy of formation
Ionization energy is the energy required to remove an electron from a gaseous atom. Electron affinity is the energy change when an electron is added. Sublimation is conversion from solid to gas, and enthalpy of formation is the overall formation from elements. .
What is the number of moles of NaCl needed to provide 0.5 moles of Cl- ions?
0.25
1.0
0.5
2.0
Each mole of NaCl yields one mole of Cl- ions upon dissociation. To get 0.5 moles of Cl-, 0.5 moles of NaCl are required. .
According to Fajans' rules, which ionic pair will have the most covalent character?
LiF
KBr
AlCl3
MgO
AlCl3 exhibits significant covalent character due to the high charge and small radius of Al3+, which polarizes Cl- electron cloud easily. Fajans' rules predict small, highly charged cations and large, polarizable anions form more covalent bonds. .
Which defect in ionic crystals involves a missing ion pair from the lattice?
Frenkel defect
Substitutional defect
Interstitial defect
Schottky defect
A Schottky defect occurs when an equal number of cations and anions are missing from the lattice, maintaining charge neutrality. A Frenkel defect involves an ion displaced to an interstitial site. Interstitial and substitutional defects refer to different solid-state phenomena. .
Which cation has the highest polarizing power?
Mg2+
Al3+
Ca2+
Na+
Polarizing power increases with higher charge and smaller ionic radius. Al3+ has the highest charge-to-size ratio among these cations, so it distorts anion electron clouds most strongly. .
Which ionic compound will exhibit the most covalent character according to Fajans' rules?
SrO
CaO
MgO
BeO
BeO shows the most covalent character because Be2+ is very small and highly polarizing, and O2- is polarizable. According to Fajans' rules, small cations with high charge create the greatest distortion of the anion. .
Which of the following has the highest percent ionic character according to Pauling's electronegativity difference?
HI
HBr
HCl
HF
HF has the greatest electronegativity difference (about 1.9) among these hydrogen halides, which yields the highest percent ionic character. Larger differences increase ionic character as per Pauling's formula. .
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Study Outcomes

  1. Identify Ionic Atoms -

    Determine which term best describes all atoms in ionic bonds and recognize that these atoms exist as ions with positive or negative charges.

  2. Differentiate Bond Types -

    Compare ionic bond questions with covalent bond basics to distinguish how electron transfer and sharing affect compound formation.

  3. Apply the Octet Rule -

    Use the octet rule quiz scenarios to predict the stability of atoms and the likelihood of ion formation during bonding.

  4. Interpret Lewis Dot Structures -

    Analyze Lewis dot structure quiz problems to visualize valence electrons and determine bond types.

  5. Analyze Charge Distribution -

    Examine how cations and anions form in ionic bonds and understand their role in creating neutral compounds.

  6. Reinforce Chemistry Concepts -

    Engage with ionic bond questions and covalent bond basics exercises to solidify your understanding and boost confidence.

Cheat Sheet

  1. Answer Spotlight: Ions as the Key Term -

    When tackling which term best describes all atoms in ionic bonds, remember that each atom becomes a charged particle - a cation or anion - commonly called an ion. According to the American Chemical Society, this electron transfer forms strong electrostatic attractions, linking oppositely charged ions into stable compounds. A quick mnemonic - "Irresistible Opposite Neighbors of Salt" - helps you recall that ions attract in ionic bonds.

  2. Octet Rule for Ionic Stability -

    The octet rule states that atoms in ionic compounds lose or gain electrons to mimic the nearest noble gas electron configuration, achieving a full valence shell. Khan Academy notes this transfer usually sees metals shedding electrons and nonmetals accepting them, creating stable cations and anions. Practice with our octet rule quiz to reinforce how many electrons each ion needs for stability.

  3. Crystal Lattice and Compound Formation -

    The Royal Society of Chemistry explains that ionic compounds form a repeating 3D crystal lattice, maximizing attractions between cations and anions while minimizing potential energy. When answering ionic bond questions, recall that each lattice point represents a formula unit, illustrating the fixed ratio of ions in the compound. Visualize a salt shaker - each grain is a neat stack of ions in a crystal structure.

  4. Drawing Lewis Dot Structures -

    The University of Sheffield's Chemguide shows that Lewis dot structures help visualize valence electrons during ionic bonding, indicating electron loss or gain with dots and arrows. Practice our Lewis dot structure quiz to master drawing cations and anions, ensuring full octets are shown for each ion. A handy tip: draw the metal first, remove its valence electrons, then bracket the ion with its new charge.

  5. Comparing Ionic and Covalent Bonds -

    While ionic bonds involve electron transfer and charged ions, covalent bond basics focus on electron sharing between atoms to form discrete molecules. The American Chemical Society highlights that polarity depends on electronegativity differences - ionic bonds typically form when the difference exceeds 2.0, whereas smaller differences yield polar or nonpolar covalent bonds. Brush up with our covalent bond basics guide to clearly contrast these bonding types.

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