Question

Give the total number of valence electrons in each of the following molecules. a. \(\mathrm{B}_{2} \mathrm{O}_{3}\) b. \(\mathrm{CO}_{2}\) c. \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\) d. \(\mathrm{NO}_{2}\)

Short answer

The total number of valence electrons for each molecule is: a. \(\mathrm{B}_{2} \mathrm{O}_{3}\): 24 b. \(\mathrm{CO}_{2}\): 16 c. \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\): 20 d. \(\mathrm{NO}_{2}\): 17

Step-by-step solution

a. Determine valence electrons of each atom in \(\mathrm{B}_{2} \mathrm{O}_{3}\) #

The molecule \(\mathrm{B}_{2} \mathrm{O}_{3}\) consists of 2 Boron (B) atoms and 3 Oxygen (O) atoms. Boron has 3 valence electrons, while Oxygen has 6 valence electrons.

a. Calculate the total valence electrons in \(\mathrm{B}_{2} \mathrm{O}_{3}\)#

To find the total valence electrons in \(\mathrm{B}_{2} \mathrm{O}_{3}\), we'll multiply the valence electrons of each atom by the number of respective atoms and then sum it up. Total valence electrons in \(\mathrm{B}_{2} \mathrm{O}_{3}\) = (2 x 3) + (3 x 6) = 6 + 18 = 24.

b. Determine valence electrons of each atom in \(\mathrm{CO}_{2}\) #

The molecule \(\mathrm{CO}_{2}\) consists of 1 Carbon (C) atom and 2 Oxygen (O) atoms. Carbon has 4 valence electrons, and Oxygen has 6 valence electrons.

b. Calculate the total valence electrons in \(\mathrm{CO}_{2}\)#

To find the total valence electrons in \(\mathrm{CO}_{2}\), we'll multiply the valence electrons of each atom by the number of respective atoms and then sum it up. Total valence electrons in \(\mathrm{CO}_{2}\) = (1 x 4) + (2 x 6) = 4 + 12 = 16.

c. Determine valence electrons of each atom in \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\) #

The molecule \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\) consists of 2 Carbon (C) atoms, 6 Hydrogen (H) atoms, and 1 Oxygen (O) atom. Carbon has 4 valence electrons, Hydrogen has 1 valence electron, and Oxygen has 6 valence electrons.

c. Calculate the total valence electrons in \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\)#

To find the total valence electrons in \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\), we'll multiply the valence electrons of each atom by the number of respective atoms and then sum it up. Total valence electrons in \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\) = (2 x 4) + (6 x 1) + (1 x 6) = 8 + 6 + 6 = 20.

d. Determine valence electrons of each atom in \(\mathrm{NO}_{2}\) #

The molecule \(\mathrm{NO}_{2}\) consists of 1 Nitrogen (N) atom and 2 Oxygen (O) atoms. Nitrogen has 5 valence electrons, and Oxygen has 6 valence electrons.

d. Calculate the total valence electrons in \(\mathrm{NO}_{2}\)#

To find the total valence electrons in \(\mathrm{NO}_{2}\), we'll multiply the valence electrons of each atom by the number of respective atoms and then sum it up. Total valence electrons in \(\mathrm{NO}_{2}\) = (1 x 5) + (2 x 6) = 5 + 12 = 17.

Key concepts

Molecular Structure

Understanding molecular structure is like piecing together a puzzle where each atom fits in a specific way to create a complete picture. Molecules are made up of atoms that are bonded together in specific arrangements. These arrangements affect the molecule's shape, size, and chemical reactivity.

• Atoms and Bonds: A molecule's overall layout depends on the number and types of atoms involved. These atoms are held together by chemical bonds that involve sharing or transferring electrons.
• Shapes Matter: The spatial arrangement of atoms in a molecule determines its molecular geometry. This geometry is crucial because it influences how molecules interact with one another and how they participate in chemical reactions.
• Predicting Structures: Chemists use models like VSEPR (Valence Shell Electron Pair Repulsion) theory to predict a molecule's structure based on the repulsions between electron pairs surrounding the central atom.

Each molecule has a unique structure that informs its properties and behavior, similar to how the layout of rooms defines a building's function.

Electron Configuration

Imagine electron configuration as the blueprint of an atom, showing precisely where the electrons reside within the atomic structure. Electrons orbit the nucleus of an atom in regions called shells, and each shell contains one or more subshells (s, p, d, f).

• Valence Electrons: Focused on just the outermost electrons of the atoms, valence electrons play a key role in chemical bonding and reactions, determining how an atom can interact with others.
• Distribution Pattern: Each element follows a unique electron configuration based on its atomic number, explained by the order of filling of these subshells (the Aufbau principle).
• Periodic Trends: Similar electron configurations lead to similar chemical properties, helping us group elements into families on the periodic table, like noble gases or alkali metals.

The way electrons are arranged in an atom dictates much of its chemical personality, influencing everything from bond formation to reactivity.

Chemical Bonding

Chemical bonding is the force that holds particles together to form compounds like water, salt, or carbon dioxide. It's crucial for understanding why atoms stick together and how new substances are created. Bonds can be classified into different types based on the nature of electron exchange or sharing.

• Ionic Bonds: Involve the transfer of electrons from one atom to another, usually between metals and non-metals, resulting in positively and negatively charged ions that attract each other.
• Covalent Bonds: Atoms share pairs of electrons. This is common in organic molecules and can involve sharing just one pair (single bond), two pairs (double bond), or even three pairs (triple bond).
• Metallic Bonds: Delocalized electrons are shared across a lattice of metal atoms, providing metals their unique properties like conductivity and malleability.

Understanding the type and nature of bonds allows chemists to deduce the properties and behaviors of various molecules in diverse environments. Whether bonds are strong or weak, flexible or rigid, defines how molecules function and interact.