Practice quiz · by a Quizcard user

Chemistry: Atomic Structure and Periodic Trends — quiz

13 multiple-choice questions covering Alkali metals, Halogens, Noble gases, Moles, Ionic bonding. One answer each; you get a score at the end and the explanation for every question. No account needed.

Updated 2026-10-24. Keys 1–4 pick an answer, Enter moves on. Redo it any time, in order or shuffled.

The questions

Answers and explanations are shown after you finish.

1. Alkali metals

   A Group 1 element is highly reactive, readily loses one electron, and forms a +1 ion. Which family does this element belong to?

   • Halogens
   • Noble gases
   • Alkali metals
   • Alkaline earth metals
2. Halogens

   Which group of elements typically gains one electron to form a -1 ion, with fluorine being the most reactive member?

   • Halogens
   • Noble gases
   • Transition metals
   • Alkali metals
3. Noble gases

   Why do elements in Group 18, such as neon and argon, rarely form chemical bonds?

   • Their valence shells are already full
   • They have very low electronegativity
   • They have the largest atomic radii in their periods
   • They readily lose electrons to form cations
4. Moles

   A chemist counts 1.204 x 10^24 particles in a sample. How many moles of the substance are present?

   • 1 mol
   • 2 mol
   • 0.5 mol
   • 6.022 mol
5. Ionic bonding

   When sodium reacts with chlorine gas, sodium transfers its valence electron to chlorine, forming Na+ and Cl- ions that attract each other. What type of bond results?

   • Polar covalent bond
   • Ionic bond
   • Covalent bond
   • Metallic bond
6. Polar covalent bonds

   In a water molecule, the oxygen atom pulls shared electrons closer to itself than the hydrogen atoms do. What causes this unequal sharing?

   • Oxygen having more neutrons than hydrogen
   • The metallic character of oxygen
   • A difference in electronegativity between O and H
   • Complete transfer of electrons from H to O
7. Metallic bonding

   Which bonding model best explains why metals conduct electricity and can be hammered into sheets without shattering?

   • Covalent bonding with shared electron pairs
   • Ionic bonding with fixed charged ions
   • Metallic bonding with delocalized electrons
   • Polar covalent bonding with partial charges
8. Atomic radius

   Sodium and chlorine are both in Period 3. Which has the larger atomic radius, and why?

   • They are equal because they are in the same period
   • Sodium, because it has fewer protons pulling on its electrons
   • Chlorine, because it has more protons
   • Chlorine, because it has more electron shells
9. Ionization energy

   Which element requires more energy to remove its outermost electron: fluorine or lithium, both in Period 2?

   • Lithium, because it has a smaller radius
   • Lithium, because it has more valence electrons
   • They require equal energy since both are in Period 2
   • Fluorine, because its increased nuclear charge holds electrons more tightly
10. Electronegativity

    A student is ranking elements by their ability to attract shared electrons in a bond. Which element should rank highest?

    • Chlorine
    • Oxygen
    • Cesium
    • Fluorine
11. Metallic character

    Between cesium and sodium, both in Group 1, which element shows greater metallic character?

    • Sodium, because it is higher on the periodic table
    • Sodium, because it has a smaller atomic radius
    • Cesium, because metallic character increases down a group
    • They are equal since both are alkali metals
12. Subatomic particles

    An atom has an atomic number of 17 and a mass number of 35. How many neutrons does it contain?

    • 35
    • 52
    • 18
    • 17
13. Isotopes

    Carbon-12 and carbon-14 both have 6 protons but different numbers of neutrons. What term describes these two atoms?

    • Allotropes
    • Isomers
    • Ions
    • Isotopes