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Quizzes > Quizzes for Business > Education

Chemistry Periodic Table Knowledge Test Quiz

Discover Periodic Table Patterns and Properties

Difficulty: Moderate
Questions: 20
Learning OutcomesStudy Material
Colorful paper art depicting elements from the chemistry periodic table for a knowledge test

This Chemistry Periodic Table Knowledge Test is a dynamic periodic table quiz that challenges learners on element symbols, atomic numbers, and trends. Ideal for students and educators seeking a targeted chemistry test, it features 15 multiple-choice questions with instant feedback. Customize this quiz freely in our quizzes editor or explore related tests like the Periodic Table Valency Quiz and the Chemistry Fundamentals Knowledge Test. Sharpen your element knowledge and elevate your chemistry understanding today!

What is the chemical symbol for Sodium?
Na
S
Sb
Sn
The chemical symbol Na comes from the Latin name natrium for sodium. It is element number 11 on the periodic table.
What is the atomic number of Oxygen?
6
7
8
16
Oxygen has eight protons in its nucleus, which gives it an atomic number of 8. This places it in period 2, group 16.
Which element has the symbol Fe?
Francium
Iron
Fermium
Fluorine
Fe stands for Ferrum, the Latin name for iron. It is atomic number 26 in the d-block of the periodic table.
Which of these elements is a noble gas?
Nickel
Nitrogen
Iodine
Neon
Neon is in group 18, the noble gases, and is chemically inert under standard conditions. The other elements belong to different groups.
Argon is located in which block of the periodic table?
f-block
s-block
p-block
d-block
Argon is element 18 and lies in group 18, which corresponds to the p-block. It completes the p orbital in its valence shell.
Which element in Period 3 has the largest atomic radius?
Argon
Aluminum
Chlorine
Sodium
Atomic radius decreases across a period due to increasing nuclear charge. Sodium, being at the left of period 3, has the largest radius.
Which element is the most electronegative?
Chlorine
Oxygen
Nitrogen
Fluorine
Fluorine has the highest electronegativity on the Pauling scale at 3.98. It readily attracts electrons in bonds.
Which element has a higher first ionization energy?
Barium
Calcium
Strontium
Magnesium
Magnesium has a smaller atomic radius and greater effective nuclear charge than calcium. This makes it harder to remove an electron.
What is the common oxidation state of Oxygen in most compounds?
-2
-1
+2
+1
Oxygen typically gains two electrons to complete its valence shell, resulting in a -2 oxidation state. This is seen in compounds like H2O and CO2.
Which of these is the electron configuration of Zinc (atomic number 30)?
[Ar]3d10 4p2
[Ar]4s2 3d8 4p2
[Ar]3d10 4s2
[Ar]4s1 3d10
Zinc fills its 3d subshell completely and has two electrons in the 4s orbital. This gives the configuration [Ar]3d10 4s2.
Which element is part of the f-block?
Platinum
Lead
Uranium
Gold
Uranium is an actinide, belonging to the f-block of the periodic table. Gold and platinum are d-block elements.
In period 4, which element marks the beginning of the d-block?
Scandium
Titanium
Potassium
Calcium
Scandium, atomic number 21, is the first element in period 4 to have its valence electrons in a d orbital. It starts the d-block.
Which of these elements is classified as a metalloid?
Calcium
Silicon
Phosphorus
Sulfur
Silicon has properties intermediate between metals and nonmetals, making it a metalloid. It lies along the metal - nonmetal dividing line.
What type of bonding is present in barium chloride (BaCl2)?
Hydrogen
Metallic
Covalent
Ionic
Barium donates two electrons to two chloride ions, forming Ba2+ and 2 Cl−. The electrostatic attraction between these ions is ionic bonding.
Which element is most likely to form a +1 ion?
Potassium
Nitrogen
Oxygen
Calcium
Potassium, an alkali metal in group 1, loses one electron to achieve a noble gas configuration. This forms K+.
Which element in group 2 has the largest atomic radius?
Magnesium
Calcium
Strontium
Beryllium
Atomic radius increases down a group as additional electron shells are added. Strontium is below calcium and thus has a larger radius.
What is the empirical formula for magnesium nitride based on valency?
Mg2N3
MgN
MgN2
Mg3N2
Magnesium has a +2 oxidation state and nitrogen has −3. To balance charges, three Mg2+ and two N3− combine to form Mg3N2.
Which element has the electron configuration [Kr]5s1?
Zinc
Strontium
Yttrium
Rubidium
Rubidium is element 37, and its single valence electron occupies the 5s orbital. This yields the configuration [Kr]5s1.
Which element is classified as a post-transition metal?
Scandium
Bromine
Manganese
Tin
Tin is in the p-block and is a metal that lies to the right of the d-block transition metals. It displays characteristics of both metals and nonmetals.
Which transition metal commonly exhibits both +2 and +3 oxidation states?
Aluminum
Neon
Calcium
Iron
Iron often forms Fe2+ and Fe3+ ions due to loss of 4s and sometimes 3d electrons. This variability is common in d-block elements.
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Learning Outcomes

  1. Identify element names, symbols, and atomic numbers
  2. Analyse periodic trends in atomic radius and electronegativity
  3. Evaluate group and period relationships for element classification
  4. Apply knowledge of valency and electron configuration to predict bonding
  5. Demonstrate understanding of s-, p-, d-, and f-block elements
  6. Master the periodic table layout and element categories

Cheat Sheet

  1. Periodic table layout - Discover how the periodic table is arranged into rows (periods) and columns (groups) to reveal recurring chemical behaviors and unlock patterns in element properties. Mastering this map helps you predict how elements will interact and how new alloys or compounds might form. Trends in the Periodic Table - RMIT University
  2. Element symbols & atomic numbers - Each element is identified by a unique symbol (like H for Hydrogen) and atomic number (1 for Hydrogen), which are essential keys for reading chemical formulas and equations. Getting comfortable with these identifiers makes balancing reactions and naming compounds a breeze. Periodic Table Trends - BYJU'S
  3. Atomic radius trends - Atomic size shrinks as you move across a period due to increased nuclear pull and expands down a group thanks to extra electron shells. Knowing these trends lets you forecast how tightly atoms hold onto their electrons, which is crucial in material design and reaction rates. Periodic Table Trends - Atomic Size - BYJU'S
  4. Electronegativity patterns - Electronegativity climbs across a period as atoms crave electrons more fiercely, and it drops down a group when added shells dull the nuclear attraction. This dance shapes bond types and molecule shapes, so it's your secret weapon in predicting reaction products. Trends in the Periodic Table - RMIT University
  5. Ionization energy trends - Removing an electron takes more energy across a period because the nucleus grips harder, but it becomes easier down a group as outer electrons sit farther away. These energy changes explain why some elements are more reactive metals or stubborn inert gases. Periodic Table Trends - Ionization Enthalpy - BYJU'S
  6. Group & period relationships - Elements in the same group share valence electron counts, so they exhibit similar chemistry, while those in the same period have equal electron shells, influencing size and reactivity. Spotting these family ties is like forecasting personalities in a social network of atoms. Periodic Table Trends - VCE Chemistry
  7. Valency & electron configuration - Atoms bond to fill or empty their outermost shells, and knowing electron configurations lets you predict how many bonds an element will form and what shapes molecules adopt. It's the blueprint for building everything from water to complex pharmaceuticals. Periodic Table Trends - BYJU'S
  8. s-, p-, d-, & f-block elements - The periodic table's blocks tell you which atomic orbitals are filling - s for shiny alkali metals, p for colorful non-metals, d for transition metals with cool catalytic powers, and f for the hidden inner-transition elements. Recognizing these blocks helps you categorize elements by behavior and applications. Periodic Table Trends - BYJU'S
  9. Metallic vs. non-metallic character - Metallic character fades across a period and strengthens down a group, while non-metallic traits do the opposite. This tug-of-war determines conductivity, luster, and whether an element will rust or form acids. Periodic Table Trends - VCE Chemistry
  10. Electron affinity trends - Electron affinity grows more negative across a period as atoms welcome extra electrons more eagerly, and it becomes less negative down a group when added distance dampens attraction. These shifts dictate whether elements act as electron grabbers or reluctant partners in bonding. Periodic Table Trends - Electron Gain Enthalpy - BYJU'S
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