Problem 56 - Chemistry Matter and Change

Question

Soda Cans The metal used to make soda cans has the electron configuration \([\mathrm{Ne}] 3 \mathrm{s}^{2} 3 \mathrm{p}^{1}\) . Identify the metal and give its group, period, and block.

Step-by-Step Solution

Answer

The metal with the electron configuration \([\mathrm{Ne}] 3 \mathrm{s}^{2} 3 \mathrm{p}^{1}\) is Aluminum (Al). It is in Group 13, Period 3, and the p-block.

Step 1: Identify the metal with the given electron configuration

To find the metal, we should first look at the electron configuration of neon which is [He] 2s^2 2p^6, and has 10 electrons. The given electron configuration of the metal is [Ne] 3s^2 3p^1 which means that there are 2 additional electrons in the 3s orbital and 1 electron in the 3p orbital. Therefore, the metal has 10 + 2 + 1 = 13 electrons. Now, we can refer to the periodic table to find the element with atomic number 13. We will find that it is Aluminum (Al).

Step 2: Determine the group, period, and block of Aluminum

Now that we have identified the metal as Aluminum (Al), we can look at the periodic table to find its group, period, and block. Group: Aluminum is in group 13 (also known as IIIA or 3A). Period: Aluminum is in period 3. Block: Aluminum is in the p-block because the last electron (3p^1) occupies a p orbital. So, the metal is Aluminum (Al) and it is in Group 13, Period 3, and p-block.

Key Concepts

Electron Configuration

Electron configuration is a way to show the distribution of electrons in an atom. It describes which orbitals the electrons occupy.
For example, the configuration \([\mathrm{Ne}] 3s^2 3p^1\) for a metal indicates that the first ten electrons are in the same arrangement as neon, a noble gas, and the remaining three electrons are distributed with two in the 3s orbital and one in the 3p orbital.
This means that the given atom has a total of 13 electrons. Knowing how to read and write electron configurations is crucial for understanding the chemical properties of elements.
It helps us predict how elements will interact with each other in chemical reactions.

Atomic Number

The atomic number of an element reflects the number of protons in its nucleus, and it uniquely identifies the element.
It also equals the number of electrons in a neutral atom, given that the number of protons and electrons are equal.
For example, when we deduced that a metal has the electron configuration \([\mathrm{Ne}] 3s^2 3p^1\), we calculated it had 13 electrons. This means the atomic number is 13.
Looking at a periodic table, the atomic number 13 corresponds to the element Aluminum (Al).

• Knowing an element's atomic number helps in determining its position on the periodic table.
• It also provides insight into its chemical properties and behavior.

Group and Period

Understanding an element’s group and period is key to predicting its chemical properties. The periodic table is organized into columns and rows, known as groups and periods, respectively.
An element's group is the column it is in, and it typically determines elements that share similar chemical traits.

• Aluminum (Al) is in group 13, sharing common characteristics with other metals in this group.
• This makes it known for properties like having three valence electrons.

Aluminum is found in period 3, which is indicated by the highest principal quantum number in its electron configuration.
The period indicates how many electron shells an element has, with Aluminum having three due to being in the third period.
Knowing group and period can help predict which elements an atom may bond with and how it might behave chemically.

p-block Elements

The periodic table is divided into blocks representing subshells being filled with electrons, including the s, p, d, and f blocks.
The p-block includes elements in groups 13 through 18.

• Elements in the p-block, like Aluminum, have their last electron enter a p orbital.
• This block contains a wide variety of elements, including nonmetals, metalloids, and metals.

The diversity of p-block elements accounts for a wide range of properties and chemical behavior.
It is significant because it helps in understanding the reactivity and chemical bonding of these elements.
Recognizing p-block elements involves looking at the electron configuration and identifying that the outermost electrons are filling the p orbitals, such as the 3p electron in Aluminum.