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Quizzes > High School Quizzes > Science

Periodic Table of Elements Practice Quiz

Master Elements, Compounds and Mixtures with Ease

Difficulty: Moderate
Grade: Grade 10
Study OutcomesCheat Sheet
Colorful paper art promoting a dynamic chemistry quiz for high school students.

This Periodic Table and compounds quiz helps you practice element symbols, groups, and simple formulas. Work through 20 quick questions to spot gaps before a test. Great for Grade 10 chemistry, and useful review for any level at school or at home.

Which of the following subatomic particles has a positive charge?
Neutron
Electron
Proton
Quark
Protons carry a positive charge and lie at the center of the atom, determining its atomic number. Electrons and neutrons do not have a positive charge, making 'Proton' the correct answer.
What does the periodic table primarily organize?
Elements by their discovery date
Elements by their cost
Elements by their state of matter
Elements by increasing atomic number
The periodic table is organized primarily by increasing atomic number, which also reflects recurring chemical properties. Other criteria mentioned do not determine the main order.
Which element is represented by the symbol O?
Hydrogen
Osmium
Oxygen
Gold
The symbol 'O' stands for Oxygen on the periodic table. The other options correspond to different element symbols and do not match the letter O.
What is the center of an atom called?
Nucleus
Mitochondria
Shell
Electron cloud
The nucleus is the central part of the atom, containing most of its mass and positive charge. The other options refer to parts of a cell or the electron distribution, making them incorrect.
Which type of bond is formed by the transfer of electrons between atoms?
Hydrogen bond
Covalent bond
Metallic bond
Ionic bond
An ionic bond forms when electrons are transferred from one atom to another, creating ions. Sharing electrons, which characterizes covalent bonds, does not describe the process in ionic bonding.
Which of the following best describes an isotope?
Atoms of the same element with different numbers of neutrons
Atoms of different elements with similar properties
Atoms that form ions
Atoms with different numbers of electrons
Isotopes are atoms of the same element that have the same number of protons but differ in the number of neutrons. The other choices do not correctly define the concept of isotopes.
What periodic trend increases as you move from left to right across a period?
Electronegativity increases
Atomic radius increases
Metallic character remains the same
Ionization energy decreases
Electronegativity, the ability of an atom to attract electrons, generally increases across a period. The other trends mentioned do not follow the same pattern.
Which element is most likely to form a +1 ion on the periodic table?
Oxygen
Sodium
Carbon
Neon
Sodium, an alkali metal, commonly loses one electron to form a +1 ion. Elements like oxygen and carbon typically form negative ions or covalent bonds, and neon is inert.
How does electron shielding affect atomic properties?
It makes atoms more radioactive
It increases effective nuclear charge
It has no effect
It decreases effective nuclear charge
Electron shielding occurs when inner electrons block the attractive force exerted by the nucleus on the outer electrons, thereby reducing the effective nuclear charge. This phenomenon impacts various atomic properties such as ionization energy and atomic radius.
Which statement correctly describes a covalent bond?
A bond formed by transferring electrons
A bond involving metal ions
A bond formed by sharing electrons between atoms
A weak bond that involves hydrogen only
A covalent bond is created when two atoms share one or more pairs of electrons. In contrast, ionic bonds involve electron transfer and other types of bonds do not accurately represent covalent sharing.
What type of chemical compound contains a metal and a non-metal?
Covalent compound
Alloy
Polymer
Ionic compound
Ionic compounds typically form between metals and non-metals, where electrons are transferred to form oppositely charged ions. The other options describe different kinds of chemical arrangements or mixtures.
In a molecule of water (H2O), what is the ratio of hydrogen atoms to oxygen atoms?
1:2
1:1
2:1
2:2
Water has two hydrogen atoms for every one oxygen atom, making the ratio 2:1. This simple stoichiometric relationship defines the composition of the water molecule.
Which property is primarily influenced by the number of electron shells in an atom?
Nuclear charge
Atomic radius
Number of protons
Electronegativity
The atomic radius is largely determined by the number of electron shells, as more shells generally mean a larger size. Electronegativity and nuclear charge are influenced by other factors, such as the effective nuclear charge and electron configuration.
What is the correct formula for sodium chloride?
NaCl
NaCl2
ClNa2
Na2Cl
Sodium chloride is composed of sodium (Na) and chlorine (Cl) in a 1:1 ratio, hence the formula NaCl. Other formulas incorrectly represent the stoichiometry of the compound.
What does the atomic number represent?
The number of electron shells
The mass of the atom
The number of protons in the nucleus
The total number of neutrons
The atomic number uniquely identifies an element by indicating the number of protons present in its nucleus. Neutrons, electron shells, and overall mass are separate properties that do not define the atomic number.
Which factor is most important in determining the type of chemical bond formed between two atoms?
Number of isotopes
Position in the periodic table
Atomic mass difference
Electronegativity difference
The difference in electronegativity between two atoms is the primary factor that decides whether they form ionic or covalent bonds. While the periodic table position provides general trends, it is the electronegativity difference that directly influences bond type.
What does a high ionization energy indicate about an element?
It easily loses electrons
It forms ionic bonds easily
It has a large atomic radius
It holds its electrons tightly
A high ionization energy means that an element requires a lot of energy to remove an electron, indicating strong attraction between the nucleus and its electrons. This makes electron loss less favorable compared to elements with lower ionization energies.
Which concept explains why elements in the same group often exhibit similar chemical behavior?
They are found in the same period
They have the same atomic mass
They have the same number of valence electrons
They have identical isotopes
Elements in the same group have similar chemical properties because they possess the same number of valence electrons, which dictates how they interact in chemical reactions. Other factors such as period location, atomic mass, or isotopic composition are not the determining reasons for similar behavior.
How does an increase in nuclear charge without additional shielding affect an atom?
It decreases the number of orbitals
It decreases the atomic radius
It has no effect
It increases the atomic radius
An increase in nuclear charge, when not offset by additional electron shielding, pulls electrons closer, leading to a decrease in atomic radius. This intensification of the electrostatic pull is the key reason behind the contraction in size.
In molecular compounds, what determines the molecule's shape?
The mass of the atoms
The ionic charges
The number of neutrons
Electron pair repulsion and bonding pairs arrangement
The molecular geometry of a compound is determined by the repulsions between electron pairs (both bonding and lone pairs) as described by the VSEPR theory. The mass of atoms, number of neutrons, or ionic charges do not dictate the spatial arrangement of atoms within a molecule.
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Study Outcomes

  1. Understand fundamental atomic structures and subatomic particle arrangements.
  2. Analyze periodic table trends and element properties.
  3. Apply concepts of chemical bonding to predict compound formations.
  4. Evaluate the relationships between elements and their compounds.
  5. Synthesize information from periodic table data to solve chemical problems.

Chemistry Quiz: Periodic Table & Compounds Cheat Sheet

  1. Structure of the Periodic Table - Dive into the layout of the periodic table by exploring rows called periods and columns known as groups. Discover how elements line up in order of increasing atomic number and why this arrangement is so clever. Get hands-on practice with the
  2. Learn First 20 Element Names and Symbols - Nail down the chemical symbols, names, atomic numbers, and masses of the first 20 elements. Knowing these basics is like having a secret code to unlock chemistry puzzles and breeze through quizzes. Reinforce your memory with the
  3. Identify Metals, Nonmetals, and Metalloids - Every element has its personality: metals are shiny and conductive, nonmetals are versatile insulators, and metalloids straddle the line. Spot where each type lives on the table and predict its behavior in reactions. Deepen your insight with the
  4. Valence Electrons and Bonding - Discover how the outermost electrons, called valence electrons, drive an element's reactivity and love to bond with others. Mastering this concept will level up your understanding of chemical formulas and compound formation. Get interactive practice with the
  5. Periodic Trends - Track how atomic radius, ionization energy, and electronegativity shift as you move across periods or down groups. These trends explain why elements behave the way they do and help you predict unknown properties. Explore the patterns in the
  6. Element Families - Meet the squads of the periodic table: alkali metals ready to explode in water, halogens lurking in salt, and noble gases keeping it chill. Learn each family's signature moves and how to recognize them at a glance. Grab the
  7. Electron Configurations - Write out the electron arrangements for elements and watch the magic of orbital filling rules come to life. This skill is key to understanding magnetic properties and chemical bonding. Drill yourself with the
  8. History of the Periodic Table - Travel back to the 1800s and follow Dmitri Mendeleev's genius in organizing elements by their properties. Discover the twists and turns that shaped the modern table and its future updates. Learn the backstory with the
  9. Worksheets and Activities - Reinforce your learning with fun puzzles, coloring pages, and timed challenges that make the elements unforgettable. Hands-on activities are the best way to commit properties and trends to memory. Download the
  10. Predict Chemical Behavior - Use an element's position to forecast how flashy or shy it will be in reactions - will it steal electrons or give them away? Practice with real-world examples like rusting iron or water splitting. Test yourself in the
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