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Quizzes > Science > Chemistry

Chemistry Unit 6 Test: How Well Do You Know Chemical Compounds?

Think you can ace our chemical compounds quiz? Dive into this chemistry quiz online and challenge your skills now!

Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art illustration for Chemistry Unit 6 quiz on chemical compounds on a coral background

Embark on a journey to master the chemistry unit 6 test and elevate your command of chemical compounds! In this interactive chemistry quiz online, you'll tackle a variety of chemical compounds quiz questions, dive deep into chemical bonding quiz scenarios, and enjoy engaging chemistry compound trivia designed to sharpen your molecular insights. As you answer each prompt, you'll boost your confidence in predicting molecular shapes, identifying bond types, and interpreting compound formulas. Need to warm up? Try our elements and compounds quiz , or review key concepts with our unit 6 chemical bonding test review . Ready to test your expertise? Take the quiz now and prove you've got what it takes!

What is the charge on a magnesium ion in MgCl2?
-1
+2
+1
-2
Magnesium loses two electrons to achieve a stable noble gas configuration, resulting in a +2 charge on Mg2+. This is typical behavior for Group 2 metals. The chloride ions each carry a -1 charge, balancing the +2 charge of magnesium. source
What type of bond forms when electrons are shared between two atoms?
Ionic bond
Covalent bond
Hydrogen bond
Metallic bond
A covalent bond forms when two atoms share one or more pairs of electrons to achieve greater stability. This type of bonding is common between nonmetal atoms. Ionic bonding, by contrast, involves transfer of electrons. source
What is the chemical formula for sodium carbonate?
NaCO2
Na3CO3
Na2CO3
NaCO3
Sodium carbonate contains two sodium ions (Na+) for each carbonate ion (CO3 2-), giving the formula Na2CO3. The 2+ charge of two sodium ions balances the 2? charge of carbonate. source
What is the molecular geometry of a molecule with two bonded atoms and no lone pairs on the central atom?
Bent
Linear
Trigonal planar
Tetrahedral
When there are two bonding pairs and no lone pairs on the central atom, the electron domains arrange 180° apart, producing a linear geometry. Carbon dioxide is a classic example. source
Which element typically forms anions by gaining one electron?
Lithium
Fluorine
Neon
Sodium
Fluorine has seven valence electrons and needs one more to complete its octet, so it readily gains one electron to form F - anions. Alkali metals like lithium and sodium lose electrons instead. source
What is the common name for H2O?
Hydronium
Hydrogen peroxide
Water
Hydroxide
H2O is universally known as water. It consists of two hydrogen atoms covalently bonded to one oxygen atom. It's the most abundant molecule in living organisms. source
In an ionic compound, electrons are:
Excited
Transferred
Delocalized
Shared equally
Ionic bonding involves the transfer of electrons from one atom (usually a metal) to another (usually a nonmetal), creating cations and anions that attract each other. This is distinct from covalent bonding. source
Which of the following is a diatomic molecule at standard conditions?
H2O
CH4
CO2
N2
Nitrogen gas (N2) exists as a diatomic molecule under normal conditions, with a strong triple bond between the two nitrogen atoms. Many other gaseous compounds are polyatomic. source
What is the approximate molar mass of H2O?
34 g/mol
44 g/mol
18 g/mol
10 g/mol
The molar mass of H2O is calculated as (2 × 1.01) + (16.00) = 18.02 g/mol. This value is used in stoichiometric and solution calculations. source
Which compound is primarily covalent in nature?
NaCl
MgO
KBr
CH4
Methane (CH4) is a covalent molecule where carbon shares electrons with hydrogen atoms. Ionic compounds like NaCl and MgO involve electron transfer, not sharing. source
Which element is the most electronegative?
Nitrogen
Oxygen
Chlorine
Fluorine
Fluorine has the highest electronegativity of all elements (3.98 on the Pauling scale), meaning it strongly attracts shared electrons in a bond. Oxygen is second highest. source
Use VSEPR theory to predict the shape of NH3.
Trigonal pyramidal
Linear
Tetrahedral
Trigonal planar
Ammonia has three bonding pairs and one lone pair on nitrogen, giving a trigonal pyramidal geometry with bond angles around 107°. source
Which molecule is polar?
H2O
CH4
CO2
BF3
Water is bent with an unequal distribution of charge, creating a net dipole moment. CO2 and BF3 are symmetric and nonpolar, while CH4 is also nonpolar. source
What is the oxidation state of sulfur in SO4 2-?
+2
+4
+6
-2
Assigning oxygen as ?2 each (4 × ?2 = ?8) and the overall charge as ?2, sulfur must be +6 to balance: x + (?8) = ?2, so x = +6. source
How many sigma bonds are present in ethene (C2H4)?
5
4
6
7
Ethene has one C=C double bond (1 sigma) and four C - H single bonds (4 sigma), for a total of 5 sigma bonds. The C=C also contains one pi bond. source
Which ion exhibits resonance in its Lewis structure?
NO3 -
CO3 2-
SO4 2-
PO4 3-
The nitrate ion (NO3 - ) has three equivalent resonance structures, each placing the double bond on a different N - O linkage. This delocalization stabilizes the ion. source
What is the hybridization of the central carbon in ethene?
sp3
sp2
dsp2
sp
In ethene, each carbon forms three sigma bonds (two C - H and one C - C) and has one unhybridized p orbital for the pi bond, corresponding to sp2 hybridization. source
What is the correct name for FeCl3?
Iron(II) chloride
Iron(IV) chloride
Iron(I) chloride
Iron(III) chloride
Iron in FeCl3 has a +3 oxidation state, so the correct systematic name is iron(III) chloride. The Roman numeral indicates the metal's oxidation number. source
What is the bond order of molecular oxygen (O2)?
3
2
1
4
Molecular oxygen has two bonding pairs and zero antibonding pairs in its valence molecular orbital diagram, giving a bond order of 2. Bond order equals (bonding electrons ? antibonding electrons)/2. source
Which factor increases the lattice energy of an ionic compound?
Smaller ionic radii
Higher temperature
Larger ionic radii
Lower ionic charges
Lattice energy is inversely proportional to the distance between ions; smaller ions allow stronger electrostatic attraction and higher lattice energies. Charge magnitude also influences it. source
What type of intermolecular force is strongest in hydrogen fluoride (HF)?
Dipole-dipole
London dispersion
Hydrogen bonding
Ionic attraction
HF molecules exhibit strong hydrogen bonding because hydrogen is bonded to a highly electronegative fluorine atom. This leads to significant dipole - dipole attraction between molecules. source
In HCl, which atom carries a partial negative charge?
Neither
Hydrogen
Chlorine
Both equally
Chlorine is more electronegative than hydrogen, so it attracts the shared electron pair more strongly and carries a partial negative charge in HCl. source
What is the hybridization of the carbon atoms in benzene?
dsp2
sp
sp2
sp3
Each carbon in benzene forms three sigma bonds and has one unhybridized p orbital that participates in the delocalized pi system, corresponding to sp2 hybridization. source
Is molecular oxygen (O2) paramagnetic or diamagnetic?
Ferromagnetic
Diamagnetic
Paramagnetic
Nonmagnetic
O2 has two unpaired electrons in its antibonding ?* orbitals, making it paramagnetic and attracted to magnetic fields. source
In a Born - Haber cycle for NaCl, what is the first step?
Ionization of Cl(g)
Formation of NaCl lattice
Sublimation of Na(s)
Dissociation of Cl2(g)
The first step is the sublimation of solid sodium to gaseous atoms (Na(s) ? Na(g)). Subsequent steps include ionization and lattice formation. source
What is the point group of a methane (CH4) molecule?
C2v
D3h
Td
Oh
Methane has tetrahedral symmetry corresponding to the Td point group, with four equivalent C - H bonds. source
What type of solid is diamond classified as?
Ionic solid
Covalent network solid
Metallic solid
Molecular solid
Diamond is a covalent network solid where each carbon atom is bonded tetrahedrally to four others in a continuous three-dimensional network. source
According to Hückel's rule, which formula describes the number of ? electrons in an aromatic compound?
2n+2
4n
4n+1
4n+2
Hückel's rule states that planar, cyclic, conjugated molecules with (4n+2) ? electrons are aromatic, leading to special stability. source
Which defect in an ionic crystal involves equal vacancies of cations and anions?
Substitutional defect
Schottky defect
Interstitial defect
Frenkel defect
A Schottky defect occurs when equal numbers of cations and anions vacate their lattice sites, maintaining electrical neutrality but creating vacancies. source
Which molten substance will conduct electricity?
NaCl
SiO2
HCl(g)
CH3Cl
Molten NaCl conducts electricity because the ions are free to move and carry charge. Covalent compounds like CH3Cl do not dissociate into ions when melted. source
What is the formal charge on nitrogen in NH4+?
+2
-1
+1
0
In NH4+, nitrogen has five valence electrons, is bonded to four hydrogens (four electrons shared), and carries no lone pairs, giving it a formal charge of zero. source
Which of the following exhibits metallic bonding?
Cu
CH4
NaCl
SiO2
Copper is a metal whose atoms share delocalized electrons in a 'sea' of electrons, characteristic of metallic bonding. Ionic, covalent network, and molecular solids do not exhibit this bonding. source
What is the coordination number of each ion in the rock salt (NaCl) crystal structure?
6
8
12
4
In the rock salt structure, each Na+ is surrounded by six Cl - ions and each Cl - by six Na+ ions, giving a coordination number of 6 for both. source
Which diatomic species is diamagnetic?
O2 2-
O2-
O2+
O2
Peroxide (O2 2-) has all electrons paired in its molecular orbitals, making it diamagnetic. In contrast, O2, O2+, and O2- have unpaired electrons. source
In the fluorite crystal structure (CaF2), what is the coordination number of the Ca2+ cation?
12
4
6
8
In CaF2, each Ca2+ is surrounded by eight F - ions in a cubic arrangement, giving a coordination number of 8. Fluorite is a common example of this coordination. source
Doping silicon with boron produces what type of semiconductor?
n-type semiconductor
Intrinsic semiconductor
p-type semiconductor
Ionic conductor
Boron has one fewer valence electron than silicon; when incorporated into the lattice it creates 'holes', leading to p-type conductivity. This is a key method in semiconductor engineering. source
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Study Outcomes

  1. Identify Bonding Types -

    Explain the differences between ionic, covalent, and metallic bonds and recognize their occurrence in various compounds.

  2. Analyze Molecular Structures -

    Interpret Lewis structures and molecular geometries to predict shape and bond angles in chemical compounds.

  3. Apply Nomenclature Rules -

    Use IUPAC guidelines to name simple inorganic compounds correctly and write their chemical formulas.

  4. Distinguish Compound Categories -

    Classify substances as acids, bases, salts, or molecular compounds based on composition and bonding.

  5. Predict Compound Properties -

    Correlate bond type and molecular structure with physical properties like melting point, solubility, and conductivity.

  6. Assess Knowledge Gaps -

    Analyze quiz results to pinpoint topics for further study and reinforce understanding of chemical compounds.

Cheat Sheet

  1. Ionic vs. Covalent Bonding -

    Review the key differences between ionic and covalent bonds: ionic compounds form from electron transfer between metals and nonmetals (e.g., NaCl), while covalent compounds share electrons between nonmetals (e.g., H₂O). A quick mnemonic is "Transfer = Ionic, Share = Covalent." According to ACS guidelines, understanding lattice energy for ionic bonds and bond enthalpy for covalent bonds is essential for predicting stability.

  2. Lewis Structures & Octet Rule -

    Practice drawing Lewis dot structures to count valence electrons and satisfy the octet (or duet for hydrogen). For example, CO₂ requires you to place double bonds on each oxygen to fulfill carbon's octet. The "Central Atom First" tip from university chemistry labs helps you assign electrons systematically.

  3. Molecular Geometry with VSEPR -

    Use the VSEPR model from IUPAC recommendations to predict shapes: AX₄ (tetrahedral), AX₃E (trigonal pyramidal), AX₂E₂ (bent), etc. Sketching a quick 3D diagram helps you visualize bond angles - 109.5° for tetrahedral, 120° for trigonal planar. This skill boosts your accuracy on structure identification questions in the chemical bonding quiz.

  4. Electronegativity & Polarity -

    Memorize the Pauling scale ranges: ΔEN > 1.7 indicates ionic character; between 0.4 and 1.7 suggests polar covalent, and < 0.4 nonpolar. For example, H - Cl (ΔEN ≈ 0.9) is polar covalent while C - H (ΔEN ≈ 0.4) is essentially nonpolar. Understanding dipole moments from research sources like the Journal of Chemical Education will guide your predictions of molecule behavior.

  5. Nomenclature & Polyatomic Ions -

    Master the IUPAC rules for naming ionic and covalent compounds and commit common polyatomic ions to memory (e.g., SO₄²❻ sulfate, NO₃❻ nitrate). A study trick is creating flashcards grouped by charge and oxygen count. This will sharpen your speed on the chemistry compound trivia and naming sections of the quiz.

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