Exploring Atomic Structure and Properties

What is the atomic mass of Carbon (C) and how is it calculated?

• 12.01 u

• 12.98 u

• 14.01 u

• 10.81 u

Define atomic number and its significance in the periodic table.

• The atomic number is the total number of electrons in an atom.

• The atomic number indicates the number of neutrons in an atom.

• The atomic number is the number of protons in an atom, significant for determining the element's identity and its position in the periodic table.

• The atomic number is the mass of an atom measured in atomic mass units.

List two isotopes of Hydrogen and their differences.

• Deuterium (2H) and Tritium (3H); Deuterium has no neutrons, while Tritium has one neutron.

• Protium (1H) and Deuterium (2H); Both isotopes have the same number of neutrons.

• Tritium (3H) and Protium (1H); Tritium has two neutrons, while Protium has one neutron.

• Protium (1H) and Deuterium (2H); Protium has no neutrons, while Deuterium has one neutron.

What is the electronic configuration of Sodium (Na)?

• 1s² 2s² 2p⁶ 3p¹

• 1s² 2s² 2p⁶ 3s¹

• 1s² 2s² 2p⁶ 3s²

• 1s² 2s² 3s¹ 3p¹

Explain the concept of valency and its importance in chemical bonding.

• Valency refers to the color of an atom in a molecule.

• Valency is the weight of an atom in grams.

• Valency is the temperature at which a substance melts.

• Valency is the measure of an atom's ability to bond with other atoms, essential for understanding chemical bonding and molecular formation.

What is the valency of Iron (Fe) in its common oxidation states?

• 1, 4

• 2, 5

• 2, 3

• 3, 4

How does the atomic mass of an element relate to its isotopes?

• The atomic mass is the weighted average of the isotopes' masses.

• The atomic mass has no relation to isotopes.

• The atomic mass is always equal to the mass of the most abundant isotope.

• The atomic mass is the sum of all isotopes' masses.

What is the atomic number of Oxygen (O) and what does it represent?

• 16

• 6

• 12

• 8

Name an isotope of Carbon and explain its use in dating.

• Carbon-14

• Carbon-15

• Carbon-12

• Carbon-13

Describe the electronic configuration of Chlorine (Cl) and its implications for reactivity.

• Chlorine has an electronic configuration of 1s² 2s² 2p⁶ 3s² 3p⁶, which leads to low reactivity.

• The electronic configuration of Chlorine is 1s² 2s² 2p⁶ 3s² 3p³, resulting in a tendency to lose electrons.

• The electronic configuration of Chlorine (Cl) is 1s² 2s² 2p⁶ 3s² 3p⁵, leading to high reactivity due to its tendency to gain one electron.

• The electronic configuration of Chlorine is 1s² 2s² 2p⁶ 3s² 3p⁴, making it very stable.