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Quizzes > Science > Chemistry

Chapter 4 Chemistry Test: Are You Ready to Ace It?

Prep for Success with Our Chemistry Unit 4 Test

Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art style chemistry quiz banner free Chapter 4 test with element symbols periodic table groups on sky blue background

This Chapter 4 Chemistry quiz helps you practice atomic structure, element properties, and periodic table groups. Work through quick, exam-style questions to spot gaps before the test, and use the unit 4 practice quiz to review tricky topics and build confidence.

Which subatomic particle carries no net electrical charge?
Positron
Proton
Neutron
Electron
Neutrons are uncharged particles found in the atomic nucleus along with protons. They play a key role in stabilizing the nucleus by offsetting electrostatic repulsion between protons. Without neutrons, many nuclei would be unstable. .
What is the chemical symbol for sodium?
S
Sd
Sn
Na
The chemical symbol 'Na' comes from the Latin name 'natrium'. It uniquely identifies sodium on the periodic table. This convention helps standardize element notation worldwide. .
Which group in the periodic table contains the noble gases?
Group 17
Group 18
Group 2
Group 1
Noble gases occupy Group 18 of the periodic table. They are characterized by having full valence electron shells. This makes them largely inert under standard conditions. .
Which of these elements is an alkali metal?
Magnesium
Potassium
Calcium
Aluminum
Alkali metals are in Group 1 of the periodic table and include lithium, sodium, and potassium. They have a single valence electron that they readily lose to form +1 cations. This makes them highly reactive, especially with water. .
What is the atomic number of carbon?
8
12
14
6
The atomic number represents the number of protons in an atom's nucleus. Carbon has 6 protons, so its atomic number is 6. This number also determines its position on the periodic table. .
Which element has the largest atomic radius?
Fluorine
Cesium
Chlorine
Helium
Atomic radius increases down a group due to added electron shells. Group 1 elements show the trend, and cesium is near the bottom. Thus, cesium has a larger radius than other listed elements. .
Which of these is a metalloid?
Boron
Sodium
Chlorine
Calcium
Metalloids have properties intermediate between metals and nonmetals. Boron sits along the dividing line on the periodic table. It exhibits both metallic and nonmetallic characteristics. .
What is the charge on an oxide ion (O)?
-1
-2
+2
+1
Oxygen typically gains two electrons to achieve a full valence shell. This results in a -2 charge for the oxide ion. This charge balances with +2 cations in many ionic compounds. .
Which of these elements is a halogen?
Bromine
Helium
Calcium
Phosphorus
Halogens occupy Group 17 of the periodic table and include fluorine, chlorine, bromine, iodine, and astatine. They have seven valence electrons and are highly reactive nonmetals. Bromine is the only liquid halogen at room temperature. .
What is the formula for calcium chloride?
Ca?Cl
CaCl?
CaCl?
CaCl
Calcium forms a +2 cation and chloride is -1. Two chloride ions are needed to balance the +2 charge. Thus the formula is CaCl?. This ionic compound is common in de-icing and food. .
Which property increases from left to right across a period?
Electron affinity
Metallic character
Atomic radius
Atomic mass
Electron affinity generally becomes more negative across a period as atoms more strongly attract electrons. Atomic radius decreases, metallic character declines, and atomic mass increases but not uniformly. The trend in electron affinity reflects increasing nuclear charge and smaller radii. .
Which element is liquid at room temperature?
Mercury
Lead
Bromine
Gallium
Mercury is the only metal that is liquid at standard room temperature and pressure. It has a low melting point due to weak metallic bonding in its d10 electron configuration. Bromine is the only halogen liquid at room temperature but is a nonmetal. .
What is the electron configuration of neon (Ne)?
1s² 2s² 2p?
1s² 2s² 2p?
1s² 2s² 3s²
1s² 2s² 2p?
Neon has 10 electrons. The filling order gives 1s² 2s² 2p? for a full second shell. This full shell explains its noble gas stability. .
Which measure of an atom indicates its ability to attract shared electrons?
Ionization energy
Atomic radius
Electron affinity
Electronegativity
Electronegativity quantifies how strongly an atom attracts bonding electrons. It increases across a period and decreases down a group. Common scales include Pauling and Mulliken. .
Which element has the highest first ionization energy?
Fluorine
Neon
Oxygen
Helium
Helium has the highest first ionization energy due to its small size and strong nuclear attraction on its two electrons. Removing one electron requires more energy than for any other element. This makes helium extremely inert. .
Which group contains elements that are all diatomic in their natural state?
Group 15
No single group
Group 16
Group 14
Diatomic elements in nature include H?, N?, O?, F?, Cl?, Br?, I?. These span multiple groups (1, 15, 16, 17). There is no single group with only diatomic elements. They form on the periodic table based on their bonding preferences. .
Which element is in the same period as sulfur but in the next group to the right?
Chlorine
Silicon
Argon
Phosphorus
Sulfur is in period 3, group 16. One group to the right is group 17 in the same period, which is chlorine. Chlorine shares period-based trends with sulfur but has one more valence electron. .
Which element's atoms have 3 valence electrons?
Aluminum
Silicon
Oxygen
Magnesium
Valence electrons are in the outermost shell. Aluminum is in group 13 and has three valence electrons. These electrons participate in bonding and determine chemistry. .
Which type of bond results from the sharing of electron pairs between atoms?
Ionic bond
Hydrogen bond
Metallic bond
Covalent bond
Covalent bonds form when atoms share electron pairs to achieve full valence shells. They are common between nonmetal atoms. Ionic bonds transfer electrons, while metallic bonds delocalize them. .
Which trend correctly describes ionization energy across a period?
Increases left to right
Random fluctuations
Stays constant
Decreases left to right
As effective nuclear charge increases across a period, electrons are held more tightly. This increases the energy required to remove an electron. Hence, first ionization energy rises left to right. .
What is the general electron configuration for p-block elements?
ns² np?
ns¹ nd¹ - ¹?
ns² np¹ - ?
ns² nd¹ - ¹?
P-block elements have valence electrons filling p orbitals. Their configurations are ns² np¹ - ? depending on group. This defines their chemical properties. .
Which force is primarily responsible for holding ionic solids together?
Dispersion forces
Metallic bonding
Dipole - dipole forces
Electrostatic attraction
Ionic solids are composed of oppositely charged ions. Electrostatic attraction between cations and anions binds the crystal lattice. This strong force leads to high melting points. .
According to Slater's rules, which electron contributes most to shielding in a multi-electron atom?
Electrons in lower shells
Electrons in the same group
Electrons in higher shells
Valence electrons only
Slater's rules approximate shielding. Electrons in inner shells are more effective at shielding than those in the same shell. This reduces the effective nuclear charge felt by outer electrons. .
Which oxide is amphoteric?
SO?
P?O?
Na?O
Al?O?
Amphoteric oxides can react both as acids and bases. Aluminum oxide reacts with acids to form salts and bases to form aluminates. This dual behavior defines amphoterism. .
Which electron configuration corresponds to the ground state of iron (Fe, atomic number 26)?
[Ar] 3d? 4s¹
[Ar] 3d? 4s²
[Ar] 3d? 4s¹
[Ar] 3d? 4s²
The Aufbau principle fills 4s before 3d. Iron's 26 electrons yield [Ar] 4s² 3d?. Exceptions occur but not for iron. This is its ground-state configuration. .
Which of these elements has the highest electronegativity?
Fluorine
Nitrogen
Oxygen
Chlorine
Fluorine is the most electronegative element on the Pauling scale. It strongly attracts bonding electrons due to its high effective nuclear charge and small radius. This makes F? very reactive. .
Which periodic trend describes the decrease in radius when a neutral atom becomes a cation?
Electron - electron repulsion increases
Effective nuclear charge decreases
Shielding effect increases
Nuclear attraction dominates
When an atom loses electrons, fewer electrons shield each other. The remaining electrons feel a higher effective nuclear charge. This pulls them closer, reducing the radius. .
Which element has the ground-state electron configuration [Kr] 5s² 4d¹? 5p²?
Indium (In)
Antimony (Sb)
Tin (Sn)
Tellurium (Te)
After krypton, the 5s and 4d orbitals fill before the 5p orbitals. Two electrons in 5p correspond to group 14. Tin (Sn) is group 14, period 5. Therefore, its configuration is [Kr] 5s² 4d¹? 5p². .
Which acid is formed when sulfur trioxide dissolves in water?
Sulfur hexafluoride (SF?)
Thiosulfuric acid (H?S?O?)
Sulfuric acid (H?SO?)
Sulfurous acid (H?SO?)
SO? reacts with water to form H?SO?. This is a strong acid known as sulfuric acid. It is widely used in industry and labs. .
Which metal forms a +3 oxidation state most commonly?
Aluminum
Calcium
Magnesium
Potassium
Aluminum commonly loses three electrons to achieve a noble gas configuration. This gives it a +3 oxidation state. Other listed metals typically form +2 or +1 states. .
Which parameter decreases when moving down a group in the periodic table?
Metallic character
Number of electron shells
Atomic radius
Ionization energy
Moving down a group adds electron shells, increasing radius and metallic character. The outer electrons are farther from the nucleus and more shielded, so ionization energy decreases. This trend is consistent across most groups. .
Which complex ion is colored due to d - d transitions?
[Fe(CN)?]³?
[Cu(NH?)?]²?
[Co(NH?)?]³?
[Ag(NH?)?]?
Copper(II) ammine complexes show blue color due to d - d electronic transitions. Ligand field splitting enables absorption in the visible region. Hexaamminecobalt(III) is low spin and may be less colored. .
According to the Aufbau principle, which orbital is filled immediately after 4p?
5p
5s
4d
3d
Aufbau filling order follows increasing n+l then n. After 4p (n+l=6) comes 5s (n+l=6, lower n). This is seen in neutral atoms like Rubidium. .
Which factor most directly affects an element's electron affinity?
Crystal structure
Atomic mass
Nuclear charge
Number of isotopes
Electron affinity depends on the attraction between nucleus and added electron. Higher nuclear charge and lower shielding increase affinity. Atomic mass or isotopes have little direct effect. .
Which metal has the highest lattice energy when forming an ionic crystal?
KBr
MgO
CsCl
NaCl
Lattice energy increases with higher charges and smaller ionic radii. MgO has +2 and - 2 ions with small radii. This produces one of the highest lattice energies among common salts. .
Which species is isoelectronic with Argon (Ar)?
K?
Cl?
Ca²?
S²?
Argon has 18 electrons. Ca²?, after losing two electrons, has 18 electrons. This makes it isoelectronic with Ar. Isoelectronic species have identical electron configurations. .
Which element exhibits an f-block filling anomaly?
Thorium
Lanthanum
Actinium
Cerium
Cerium can exhibit 4f¹5d¹6s² instead of expected 4f²6s². This anomaly arises from close energies of 4f and 5d orbitals. Many f-block elements show such irregular configurations. .
Which is the correct order of acidity for the oxides: CO?, SiO?, Al?O??
CO? > SiO? > Al?O?
SiO? > CO? > Al?O?
Al?O? > SiO? > CO?
CO? > Al?O? > SiO?
Acidity of oxides increases with element electronegativity and oxidation state. CO? is acidic, SiO? is weakly acidic, and Al?O? is amphoteric. Thus, CO? > SiO? > Al?O?. .
Which is the paramagnetic species?
Zn²?
Cu?
Cd²?
Fe²?
Paramagnetic species have unpaired electrons. Fe²? has configuration [Ar]3d?, with four unpaired electrons in high-spin complexes. Zn²? and Cd²? have filled d-subshells and are diamagnetic. .
Which energy change corresponds to removing an electron from a gaseous atom?
Lattice energy
Electron affinity
First ionization energy
Enthalpy of vaporization
First ionization energy is defined as the energy required to remove the outermost electron from a neutral gaseous atom. It is an endothermic process. Electron affinity refers to adding an electron, not removing one. .
Which principle explains why two electrons in the same orbital must have opposite spins?
Pauli exclusion principle
Heisenberg uncertainty principle
Aufbau principle
Hund's rule
The Pauli exclusion principle states that no two electrons in an atom can have the same set of four quantum numbers. In one orbital, two electrons must have opposite spins (ms = +½ and - ½). This rule underpins electronic structure. .
Which oxide of nitrogen is neutral in water (neither acidic nor basic)?
NO?
NO
N?O
N?O?
Nitric oxide (NO) is relatively insoluble and does not form acids or bases in water. Other oxides like NO? form nitrous/nitric acids. N?O is also called laughing gas and has minimal acid-base behavior. .
Which quantum number indicates the shape of an orbital?
Magnetic quantum number (m?)
Spin quantum number (m?)
Principal quantum number (n)
Azimuthal quantum number (l)
The azimuthal (angular momentum) quantum number l defines orbital shape (s, p, d, f corresponding to l = 0,1,2,3). It also affects energy in multi-electron atoms. Principal n sets shell, m? orientation, and m? spin. .
Which halogen oxide is used as a bleaching agent in water treatment?
ClO?
ClO?
Cl?O?
Cl?O
Chlorine dioxide (ClO?) is an effective bleach and disinfectant used in water treatment. It has strong oxidizing properties without forming chlorinated by-products. Other oxides are less stable or less effective. .
Which coordination number is most common for transition metal complexes following the 18-electron rule?
4
6
8
10
Many transition metal complexes achieve 18 valence electrons with an octahedral (coordination number 6) geometry. This arrangement provides strong ligand field stabilization. Tetrahedral (4) and other coordination numbers occur but less frequently under the 18-electron rule. .
Which element has a half?filled d?subshell configuration?
Cr (Chromium)
Mn (Manganese)
Fe (Iron)
Cu (Copper)
A half-filled d?subshell has five electrons in five orbitals. Manganese has configuration [Ar] 3d? 4s². This half-filling confers extra stability. Chromium has [Ar] 3d? 4s¹, which is not strictly half?filled d only. .
Which phenomenon explains why copper and gold are colored while silver is not prominently colored?
Higher ionization energy
Surface plasmon resonance
Electron affinity difference
Lattice energy variation
Surface plasmon resonance involves collective oscillation of conduction electrons interacting with light. Copper and gold's d-band absorption yields distinct colors. Silver's plasmon frequency falls in UV, making it reflect visible light neutrally. .
Which is the correct expression for the Born - Haber cycle relation of lattice energy (U)?
?Hf = U - IE - EA
?Hf = ?Hsub + U - IE - EA
?Hf = ?Hsub + IE + EA + U + ?Hion
?Hf = IE + EA + U + ?Hsub
The Born - Haber cycle breaks down formation enthalpy (?Hf) into sublimation (?Hsub), ionization energy (IE), electron affinity (EA), ionic bond enthalpy (?Hion), and lattice energy (U). All terms sum to ?Hf. This allows solving for U. .
Using Slater's rules, calculate the effective nuclear charge (Z_eff) felt by a 3p electron in sulfur (Z=16).
9.0
8.4
7.2
6.0
Slater's rules assign shielding constants: same n-group electrons shield by 0.35, n - 1 by 0.85, and lower by 1.00. For S 3p: Z_eff ? 16 - (7 ×0.35 + 8×0.85) ? 7.2. This effective charge influences many properties. .
Predict the magnetic moment (in BM) of a high-spin d? complex.
5.92 BM
4.90 BM
3.87 BM
0 BM
High-spin d? has five unpaired electrons. Magnetic moment ? = ?(n(n+2)) BM. For n=5, ? ? ?35 ? 5.92. This parameter helps characterize complexes. .
Calculate the percentage ionic character of a bond with ?? (Pauling) = 1.2.
45%
22%
38%
33%
Pauling's formula: % ionic = (1 - e^( - 0.25(??)²)) ×100. Substituting ??=1.2 gives ?(1 - e^ - 0.36)×100?38%. This quantifies bond polarity. .
Which principle limits simultaneous precision of momentum and position measurements?
Hund's rule
Pauli exclusion principle
Heisenberg uncertainty principle
Aufbau principle
The Heisenberg uncertainty principle states that ?x·?p ? ?/2. This sets a fundamental limit on simultaneously measuring an electron's position and momentum. It underlies quantum mechanical behavior. .
Using Born - Haber data, which factor most increases lattice energy: higher ionic charge or smaller ionic radius?
Lower ionic charge
Smaller ionic radius
Higher ionic charge
Larger ionic radius
Lattice energy is proportional to (chargeproduct)/distance. Doubling ionic charges quadruples lattice energy, while halving radius only doubles it. Thus, charge has a stronger effect. .
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Study Outcomes

  1. Understand Element Properties -

    Explain key characteristics of elements, including atomic number, atomic mass, and electron configuration, to reinforce core chemistry unit 4 test concepts.

  2. Identify Periodic Table Groups -

    Classify elements into their respective families and groups based on shared properties and periodic trends in the chapter 4 test.

  3. Apply Knowledge in a Practice Quiz -

    Use the free Chapter 4 test to solve targeted questions that mirror exam-style prompts and test your chemistry study guide chapter 4 understanding.

  4. Analyze Quiz Performance -

    Review your results to pinpoint strengths and weaknesses, enabling a strategic study plan for the upcoming chemistry test unit 4.

  5. Target Areas for Improvement -

    Recognize specific topics that need more review and access focused explanations to close knowledge gaps before the real exam.

  6. Boost Exam Confidence -

    Track your progress over multiple attempts, build mastery through repetition, and approach your Chapter 4 test with greater assurance.

Cheat Sheet

  1. Periodic Table Organization -

    Familiarize yourself with the layout of periods (rows) and groups (columns) as defined by IUPAC; elements in the same group share similar valence electron configurations and chemical behaviors. Recognizing that Group 1 elements are alkali metals and Group 17 are halogens will help you navigate questions on your chapter 4 test effortlessly.

  2. Electron Configuration Rules -

    Review Aufbau's principle, Hund's rule, and the Pauli exclusion principle to predict ground-state electron configurations (e.g., Fe: [Ar] 4s² 3d❶) as detailed in UC Berkeley's ChemWiki. A quick mnemonic "1s before 2s, fill p's last" can speed up writing configurations on your chemistry unit 4 test.

  3. Periodic Trends: Atomic Radius & Ionization Energy -

    Learn that atomic radius increases down a group and decreases across a period, while first ionization energy does the opposite, as illustrated in the Royal Society of Chemistry's trend diagrams. Mnemonic "AR down & left, IE up & right" helps solidify these patterns for the chemistry study guide chapter 4 questions.

  4. Element Classification -

    Differentiate metals, nonmetals, and metalloids using the diagonal "staircase" on the table; metals (left) are generally conductive and lustrous, nonmetals (right) are insulators, and metalloids exhibit mixed traits (source: Khan Academy). Remember that elements along the staircase line often show intermediate behavior, a key concept for classification items on the chapter 4 test.

  5. Valence Electrons & Reactivity Patterns -

    Count valence electrons to predict reactivity: Group 1 metals (one valence electron) form +1 ions, while halogens (seven valence electrons) form - 1 ions, as per IUPAC guidelines. Knowing this will aid you in answering reaction and bonding questions quickly during the chemistry test unit 4 quiz.

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