Grade 9 Chemistry Self Test

Which of the following properties generally INCREASES from left to right across a period in the periodic table?

• Atomic radius

• Ionization energy

• Metallic character

• Number of electron shells

Which element has the highest electronegativity?

• Fluorine (F)

• Chlorine (Cl)

• Francium (Fr)

• Oxygen (O)

As you move down a group in the periodic table, atomic radius generally:

• Increases

• Decreases

• Remains constant

• Shows no consistent trends

Which of these elements would be expected to have the largest ionic radius?

• Li⁺

• Na⁺

• K⁺

• Rb⁺

Which of the following elements has the lowest first ionization energy?

• Helium (He)

• Sodium (Na)

• Neon (Ne)

• Argon (Ar)

Electron affinity is best defined as the:

• Energy required to remove an electron from an atom.

• Tendency of an atom to attract electrons towards itself in a chemical bond.

• Energy released or absorbed when an electron is added to a neutral atom.

• Energy difference between the highest occupied and lowest unoccupied energy levels.

Which of these elements exhibits the most metallic character?

• Carbon (C)

• Silicon (Si)

• Germanium (Ge)

• Tin (Sn)

Which of the following is a TRUE statement about electronegativity?

• It is the same as electron affinity.

• It only applies to ionic bonds.

• It is a measure of an atom's ability to attract shared electrons in a covalent bond.

• It increases down a group in the periodic table.

Elements in the same group (vertical column) of the periodic table share similar chemical properties. This is primarily because they have the same:

• Number of protons

• Atomic mass

• Number of valence electrons

• Number of neutrons

Which of the following correctly explains the general trend of ionization energy in the periodic table?

• Increases across a period due to increasing nuclear charge.

• Decreases down a group due to increasing shielding effect.

• Both a and b

• Neither a nor b