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Quizzes > Science

Periodic Table Families Quiz: Identify Element Groups

Quick, free periodic table groups quiz. Instant results.

Editorial: Review CompletedCreated By: Lucas LinderUpdated Aug 28, 2025
Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art periodic table with colorful element group labels on sky blue background promoting families quiz

This periodic table families quiz helps you spot each element's group and the trends they share. Work through quick questions to match names, main groups, and common properties, with instant feedback. For extra practice, try our periodic table quiz, build skills with the valence electrons quiz, or review key shorthand in periodic table symbols.

Which group on the periodic table is known as the noble gases?
Group 1
Group 17
Group 18
Group 2
The noble gases occupy group 18 and are characterized by a full valence shell, making them largely inert under normal conditions. They include helium, neon, argon, krypton, xenon, and radon. Their lack of chemical reactivity stems from having complete electron configurations. .
What family does sodium belong to?
Alkali metals
Noble gases
Halogens
Alkaline earth metals
Sodium is an alkali metal found in group 1 of the periodic table. Alkali metals have a single valence electron which they readily lose to form +1 cations. This makes them highly reactive, especially with water. .
Which element is the lightest alkali metal?
Rubidium
Potassium
Lithium
Sodium
Lithium has the lowest atomic number (3) among the alkali metals, making it the lightest member of group 1. It has one valence electron, which contributes to its high reactivity. Lithium's low density and unique properties make it useful in batteries. .
Which group contains the halogens?
Group 17
Group 2
Group 13
Group 14
The halogens are located in group 17 and include fluorine, chlorine, bromine, iodine, and astatine. These elements have seven valence electrons and typically form -1 anions. Their high electronegativity makes them very reactive, especially with alkali metals. .
What is the chemical symbol for the alkaline earth metal magnesium?
Mo
Ag
Mn
Mg
Magnesium is an alkaline earth metal with the symbol Mg and atomic number 12. It has two valence electrons and commonly forms a +2 oxidation state. Magnesium is abundant in the Earth's crust and essential for biological processes. .
Which of these elements is a noble gas?
Niobium
Nickel
Nitrogen
Neon
Neon is a noble gas with atomic number 10, occupying group 18 of the periodic table. Like other noble gases, neon has a full valence shell and exhibits very low chemical reactivity. It is commonly used in neon lighting. .
To which family does calcium belong?
Halogens
Alkaline earth metals
Noble gases
Alkali metals
Calcium is an alkaline earth metal in group 2, characterized by having two valence electrons which it tends to lose to form a +2 cation. This family includes beryllium, magnesium, calcium, strontium, barium, and radium. They are shiny, silvery-white, and somewhat reactive at standard conditions. .
What is the group number for the alkali metals?
Group 18
Group 2
Group 1
Group 17
Alkali metals occupy group 1 of the periodic table. They contain a single valence electron, which they readily lose to form +1 ions. This group includes lithium, sodium, potassium, rubidium, cesium, and francium. .
Which element in the halogen family is a liquid at room temperature?
Fluorine
Chlorine
Bromine
Iodine
Bromine is the only nonmetallic element that is a liquid at room temperature and belongs to group 17. It has a reddish-brown color and emits a strong odor. Its reactivity is between that of chlorine and iodine. .
What is the general valence electron count for group 2 elements?
2
8
7
1
Group 2 elements, known as alkaline earth metals, have two valence electrons in their outer shell. They commonly lose these electrons to form +2 cations. This electron configuration contributes to their moderate reactivity. .
Which of these elements is a chalcogen?
Helium
Sulfur
Carbon
Oxygen
Chalcogens are the elements in group 16, which include oxygen, sulfur, selenium, tellurium, and polonium. Oxygen is the lightest and most abundant chalcogen. These elements typically form -2 anions. .
Which family is characterized by having a full valence shell?
Lanthanides
Halogens
Noble gases
Alkali metals
Noble gases have a complete set of valence electrons, giving them stable electron configurations. This full valence shell accounts for their very low chemical reactivity. They are found in group 18 of the periodic table. .
Which element is a p-block element in group 13?
Iron
Magnesium
Potassium
Aluminum
Aluminum is located in group 13 of the p-block and has the electron configuration [Ne]3s2 3p1. It commonly exhibits a +3 oxidation state. Aluminum is the most abundant metal in the Earth's crust. .
Which group contains elements that commonly have a +3 oxidation state?
Group 16
Group 15
Group 13
Group 14
Elements in group 13 typically lose three electrons to achieve a stable noble gas configuration, resulting in a +3 oxidation state. This family includes boron, aluminum, gallium, indium, and thallium. Their chemistry reflects this common valence. .
Which element is a metalloid in group 14?
Lead
Tin
Carbon
Silicon
Silicon is a metalloid found in group 14 with the electron configuration [Ne]3s2 3p2. It exhibits properties intermediate between metals and nonmetals. Silicon's semiconducting behavior is key in electronic devices. .
Which series includes the elements from atomic numbers 57 to 71?
Post-transition metals
Transition metals
Lanthanides
Actinides
The lanthanide series comprises elements with atomic numbers 57 (lanthanum) through 71 (lutetium). They are f-block elements characterized by filling of 4f orbitals. Lanthanides exhibit similar chemical properties due to their electron configurations. .
Which of the following is not a characteristic of alkali metals?
One valence electron
High melting points
Form +1 cations
React with water
Alkali metals actually have low melting points compared to most metals. They possess one valence electron and readily form +1 cations, reacting vigorously with water. Their softness and low density are also notable properties. .
Which group of transition metals is known as the coinage metals?
Group 9
Group 10
Group 11
Group 12
The coinage metals - copper, silver, and gold - are located in group 11. They have been used historically for currency due to their malleability and resistance to corrosion. Their filled d-subshells contribute to their characteristic metallic luster. .
Which element is the heaviest naturally occurring element in the actinide series?
Uranium
Thorium
Neptunium
Protactinium
Uranium, atomic number 92, is the heaviest actinide that occurs naturally in appreciable quantities. Neptunium and plutonium can be found in trace amounts, but are primarily synthetic. Uranium's radioactivity has made it central to nuclear energy. .
In what group would you find elements that have an s2p1 valence electron configuration?
Group 13
Group 14
Group 15
Group 12
Elements in group 13 have the general valence electron configuration s2p1, totaling three valence electrons. This leads them to commonly exhibit +3 oxidation states. The boron group is the first p-block family on the periodic table. .
Which of the following pairs are both pnictogens?
Nitrogen and Phosphorus
Oxygen and Sulfur
Fluorine and Chlorine
Carbon and Silicon
Pnictogens are elements in group 15, including nitrogen, phosphorus, arsenic, antimony, and bismuth. Nitrogen and phosphorus are the two lightest pnictogens. They characteristically form -3 anions in many compounds. .
Which group's elements are most likely to form a -2 anion?
Group 12
Group 14
Chalcogens (Group 16)
Halogens (Group 17)
Chalcogens in group 16 have six valence electrons and tend to gain two electrons to fill their valence shell, forming -2 anions. Oxygen and sulfur are common examples. This tendency underlies many oxide and sulfide minerals. .
Which element is the first actinide to commonly exhibit a +6 oxidation state?
Protactinium
Uranium
Thorium
Neptunium
Uranium is the first actinide that frequently shows a +6 oxidation state, especially in the uranyl ion (UO2)2+. This oxidation state is key in nuclear fuel chemistry and environmental studies. Earlier actinides like thorium prefer +4. .
The inert pair effect becomes more pronounced in which group of the periodic table?
Group 14
Group 16
Group 13
Group 15
The inert pair effect refers to the reluctance of the outermost s-electrons to participate in bonding, most evident in the heavier p-block elements of group 13. For example, thallium commonly forms +1 rather than +3. This effect increases down the group due to relativistic stabilization. .
What underlying cause leads to the lanthanide contraction observed across the lanthanide series?
Addition of d-orbitals
Relativistic effects only
Decrease in atomic mass
Increased nuclear charge with poor f-electron shielding
Lanthanide contraction arises because as protons are added across the series, the poorly shielding 4f electrons fail to offset the increased nuclear charge, causing a gradual decrease in ionic and atomic radii. This affects the chemistry of subsequent elements. Relativistic effects also contribute but are secondary. .
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Study Outcomes

  1. Identify Element Families -

    Define what a family on the periodic table is and pinpoint the major groups (e.g., alkali metals, halogens) in the periodic table in families quiz.

  2. Analyze Periodic Trends -

    Examine how properties like atomic radius and ionization energy change across and down the periodic table of families to reveal underlying patterns.

  3. Classify Elements Correctly -

    Sort elements into their correct families based on shared characteristics such as valence electron count and reactivity.

  4. Compare Family Characteristics -

    Contrast the chemical and physical properties of different element families and explain what drives their similarities and differences.

  5. Apply Quiz Strategies -

    Use your understanding of element families to confidently tackle quiz questions and reinforce your mastery of the periodic table in families.

Cheat Sheet

  1. Groups vs. Periods: Defining Families -

    In the periodic table in families, elements are arranged into vertical columns called groups (or families) and horizontal rows called periods. Groups contain elements with the same number of valence electrons, which drives similar chemical behavior, whereas periods track increasing atomic number. Recognizing this layout helps answer "what is family on the periodic table" by focusing on columns, not rows.

  2. Valence Electrons and Chemical Trends -

    Family members share valence-electron configurations, so elements in Group 1 all have a single valence electron, making them highly reactive (IUPAC). Trends such as ionization energy and atomic radius shift predictably down a group, guiding you when forecasting reactivity. A handy mnemonic: "Aunt Sally Loves Bananas" reminds you that Alkali (A) metals (S) in the first group (L) are superreactive (B).

  3. Alkali and Alkaline Earth Metals -

    Group 1 (alkali metals) and Group 2 (alkaline earth metals) illustrate how increasing principal quantum levels boost atomic radius and reactivity (Royal Society of Chemistry). For example, potassium (K) is more reactive than sodium (Na) due to its larger atomic size. Remember: "Down the group, more reactive proves true."

  4. Halogens to Noble Gases -

    Group 17 elements (halogens) possess seven valence electrons, making them highly electronegative and eager to gain one more (Pauling scale). In contrast, Group 18 (noble gases) have full valence shells and are mostly inert, which exemplifies why families define reactivity patterns. A quick trick: "Freaky Clowns Bring In Real Atmosphere" for F, Cl, Br, I, Rn.

  5. d-Block Dynamics: Transition Metals -

    Transition metals span groups 3 - 12 and show variable oxidation states thanks to partially filled d orbitals, enabling colorful complexes and catalytic properties (American Chemical Society). Unlike main-group families, these elements can lose different numbers of electrons, so you'll often see Fe²❺ and Fe³❺ in reactions. Visualize their electron configurations to master "what's a family on the periodic table" in the d-block context.

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