How many valence electrons does each of the following atoms have? a. rubidium,
b. arsenic,
c. aluminum,
d. nickel,
The Corr
The Correct Answer and Explanation is:
e
Correct Answers:
a. Rubidium (Rb) – 1 valence electron
b. Arsenic (As) – 5 valence electrons
c. Aluminum (Al) – 3 valence electrons
d. Nickel (Ni) – 2 valence electrons
Explanation:
Valence electrons are the electrons located in the outermost energy level (shell) of an atom. These electrons are the most involved in chemical bonding and determine how an element reacts chemically.
To determine the number of valence electrons, we look at the element’s position in the periodic table, specifically its group (column). Elements in the same group have the same number of valence electrons.
a. Rubidium (Rb) is in Group 1 and Period 5 of the periodic table. Group 1 elements are known as alkali metals and all have one valence electron. This electron is located in the 5s orbital, making rubidium highly reactive and eager to lose that single electron to form a stable configuration.
b. Arsenic (As) is in Group 15 and Period 4. Group 15 elements have five valence electrons. These electrons are found in the 4s and 4p orbitals. Arsenic commonly forms covalent bonds by sharing its valence electrons to achieve a full octet.
c. Aluminum (Al) belongs to Group 13 and Period 3. Group 13 elements have three valence electrons. Aluminum has these electrons in the 3s and 3p orbitals. It often loses all three valence electrons to form a +3 charge in ionic compounds.
d. Nickel (Ni) is in Group 10 and Period 4. While transition metals are more complex due to their d-electrons, nickel usually has two valence electrons, typically found in the 4s orbital. These two electrons are commonly involved in bonding, while its 3d electrons may also participate depending on the chemical context.
Understanding valence electrons is essential because they govern the chemical behavior and reactivity of elements.
ct Answer and Explanation is: