Question

For each of the following metals, how many electrons will the metal atoms lose when the metal reacts with a nonmetal? a. sodium b. potassium c. magnesium d. barium e. aluminum

Short answer

The metals will lose the following number of electrons when reacting with a nonmetal: a. Sodium: 1 electron b. Potassium: 1 electron c. Magnesium: 2 electrons d. Barium: 2 electrons e. Aluminum: 3 electrons

Step-by-step solution

Look up metal electron configurations

Look up the electron configurations of the following metals: sodium, potassium, magnesium, barium, and aluminum. You can find this information using a periodic table.

Determine the number of electrons in the outer shell

Identify the number of valence electrons (electrons in the outermost shell) for each metal. These are the electrons that the metal will lose when it reacts with a nonmetal. a. Sodium (Na): Electron configuration: \(1s^2 2s^2 2p^6 3s^1\). Valence electrons: 1 electron in the 3s orbital. Sodium will lose 1 electron when reacting with a nonmetal. b. Potassium (K): Electron configuration: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^1\). Valence electrons: 1 electron in the 4s orbital. Potassium will lose 1 electron when reacting with a nonmetal. c. Magnesium (Mg): Electron configuration: \(1s^2 2s^2 2p^6 3s^2\). Valence electrons: 2 electrons in the 3s orbital. Magnesium will lose 2 electrons when reacting with a nonmetal. d. Barium (Ba): Electron configuration: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^2\). Valence electrons: 2 electrons in the 6s orbital. Barium will lose 2 electrons when reacting with a nonmetal. e. Aluminum (Al): Electron configuration: \(1s^2 2s^2 2p^6 3s^2 3p^1\). Valence electrons: 3 electrons (2 in the 3s orbital and 1 in the 3p orbital). Aluminum will lose 3 electrons when reacting with a nonmetal.

Summarize results

The metals will lose the following number of electrons when reacting with a nonmetal: a. Sodium: 1 electron b. Potassium: 1 electron c. Magnesium: 2 electrons d. Barium: 2 electrons e. Aluminum: 3 electrons

Key concepts

Electron Configuration

Electron configuration is a way to describe the arrangement of electrons around an atom's nucleus. It helps us understand how atoms bond and react with each other. Electrons are arranged in shells or energy levels, each with specific sublevels and orbitals.
- Each shell has a set number of sublevels (s, p, d, f).- Each sublevel has a certain number of orbitals that can hold two electrons.
The configuration is usually written as a sequence of numbers and letters. For example, sodium, with an electron configuration of \(1s^2 2s^2 2p^6 3s^1\), has its outermost electron in the 3s orbital. Knowing the electron configuration helps to predict which electrons will be lost first in reactions.

Metal Reactivity

Metal reactivity refers to how easily a metal atom loses electrons during a reaction, often resulting in the formation of positive ions or cations. Metals at the start of the periodic table, like sodium and potassium, are highly reactive because they have only one electron in their outer shell.
i. Metals with fewer valence electrons tend to lose them more easily, making them more reactive. - Reactivity is influenced by the electron configuration.
Highly reactive metals like potassium can violently react with water or air, making them important to handle safely in chemical experiments.

Periodic Table

The periodic table is a crucial tool for understanding the properties of elements, including metals, nonmetals, and metalloids. It is arranged in a way that reflects the structure of atoms, especially focusing on electron configuration.
- Elements in the same column or group have similar valence electron configurations. - Metals are generally to the left and middle of the table.
The position of an element in the periodic table helps to determine its electron configuration as well as its overall reactivity. For instance, sodium and potassium are both in group 1, indicating they have one valence electron and follow similar chemical behaviors.

Valence Shell

The valence shell is the outermost shell of an atom, and it determines how an atom interacts chemically with other atoms. For metals, the number of electrons in the valence shell is a key determinant of reactivity.
- Valence electrons are the electrons available for bonding and chemical reactions. - The fewer valence electrons a metal has, the more reactive it can be, as seen with sodium and potassium.
In contrast, metals like magnesium and barium have more valence electrons, making them slightly less reactive as they require more energy to remove these additional electrons.

Chemical Reactions

Chemical reactions involve the rearrangement of atoms and electrons between substances to form new compounds. Metals play a critical role in these reactions due to their tendency to lose electrons easily.
- During a reaction, metals lose electrons, which can then be gained by nonmetals. - This electron transfer leads to the creation of ionic compounds, like when sodium reacts with chlorine to form sodium chloride (NaCl).
Understanding electron configurations and valence shells allows chemists to predict and manipulate chemical reactions, ensuring desired products are formed efficiently and safely.