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Magazine Chapter 8: Problem 77
Write the charge and full ground-state electron configuration of the monatomic ion most likely to be formed by each: (a) Al (b) S (c) Sr
Short Answer
Expert verified
Al鲁鈦�: [Ne], S虏鈦�: [Ar], Sr虏鈦�: [Kr]
Step by step solution
01
Determine the charge of the ion for Al
Aluminum (Al) is in group 13 of the periodic table. Elements in group 13 typically lose three electrons to form cations with a +3 charge. Therefore, the monatomic ion formed by Al is Al鲁鈦�.
02
Write the electron configuration for neutral Al
The atomic number of Al is 13, which means it has 13 electrons in its neutral state. The electron configuration for neutral Al is: \[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^1 \]
03
Write the electron configuration for Al鲁鈦�
To form Al鲁鈦�, aluminum loses three electrons. The electrons are removed from the outermost shell (3s and 3p orbitals). Thus, the electron configuration for Al鲁鈦� is: \[ 1s^2 \, 2s^2 \, 2p^6 \]
04
Determine the charge of the ion for S
Sulfur (S) is in group 16 of the periodic table. Elements in group 16 typically gain two electrons to form anions with a -2 charge. Therefore, the monatomic ion formed by S is S虏鈦�.
05
Write the electron configuration for neutral S
The atomic number of S is 16, which means it has 16 electrons in its neutral state. The electron configuration for neutral S is: \[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^4 \]
06
Write the electron configuration for S虏鈦�
To form S虏鈦�, sulfur gains two electrons. Therefore, the electron configuration for S虏鈦� is: \[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \]
07
Determine the charge of the ion for Sr
Strontium (Sr) is in group 2 of the periodic table. Elements in group 2 typically lose two electrons to form cations with a +2 charge. Therefore, the monatomic ion formed by Sr is Sr虏鈦�.
08
Write the electron configuration for neutral Sr
The atomic number of Sr is 38, which means it has 38 electrons in its neutral state. The electron configuration for neutral Sr is: \[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^{10} \, 4p^6 \, 5s^2 \]
09
Write the electron configuration for Sr虏鈦�
To form Sr虏鈦�, strontium loses two electrons. The electrons are removed from the outermost shell (5s orbital). Thus, the electron configuration for Sr虏鈦� is: \[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^{10} \, 4p^6 \]
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
electron configuration
Electron configuration is a method that shows the distribution of electrons around the nucleus of an atom. This is essential for understanding how elements interact and bond with each other. Electrons are arranged in specific energy levels, or shells, and sublevels (s, p, d, f). For instance, the ground-state electron configuration of a neutral aluminum (Al) atom is \[ 1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^1 \]. This notation indicates that an aluminum atom has a total of 13 electrons, filling these sublevels in sequence according to the Aufbau principle and Hund's rule.
periodic table groups
The periodic table groups elements by their chemical properties and electron configurations. Elements in the same group have similar properties due to their similar valence electron configurations. For example:
- Group 1 elements (alkali metals) have one valence electron.
- Group 2 elements (alkaline earth metals) have two valence electrons.
Understanding these groups helps us predict the behavior of elements. Aluminum (Al) is in group 13 and typically loses three electrons to become Al鲁鈦�. Sulfur (S) is in group 16 and often gains two electrons to form S虏鈦�. Strontium (Sr) belongs to group 2 and loses two electrons to become Sr虏鈦�.
- Group 1 elements (alkali metals) have one valence electron.
- Group 2 elements (alkaline earth metals) have two valence electrons.
Understanding these groups helps us predict the behavior of elements. Aluminum (Al) is in group 13 and typically loses three electrons to become Al鲁鈦�. Sulfur (S) is in group 16 and often gains two electrons to form S虏鈦�. Strontium (Sr) belongs to group 2 and loses two electrons to become Sr虏鈦�.
ion charge determination
Determining the charge of an ion involves understanding how many electrons are lost or gained by the atom. Atoms lose or gain electrons to achieve a stable electron configuration, often resembling the nearest noble gas. Examples include:
- Aluminum (Al), with 3 valence electrons, loses three to form Al鲁鈦�.
- Sulfur (S), with 6 valence electrons, gains two to complete its outer shell, forming S虏鈦�.
- Strontium (Sr) loses two electrons to attain the electron configuration of krypton (Kr), forming Sr虏鈦�.
This trend follows the octet rule, where atoms strive to have eight electrons in their valence shell.
- Aluminum (Al), with 3 valence electrons, loses three to form Al鲁鈦�.
- Sulfur (S), with 6 valence electrons, gains two to complete its outer shell, forming S虏鈦�.
- Strontium (Sr) loses two electrons to attain the electron configuration of krypton (Kr), forming Sr虏鈦�.
This trend follows the octet rule, where atoms strive to have eight electrons in their valence shell.
aluminum ion
An aluminum ion (Al鲁鈦�) is formed when aluminum loses three electrons. This loss is because aluminum wants to achieve a stable electron configuration similar to that of the noble gas neon (Ne). The electron configuration of a neutral aluminum atom is \[ 1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^1 \]. When it becomes Al鲁鈦�, the configuration changes to \[ 1s^2 \ 2s^2 \ 2p^6 \], effectively removing the electrons from the 3s and 3p orbitals. This cation formation explains why aluminum commonly has a +3 charge.
sulfur ion
A sulfur ion (S虏鈦�) is created when sulfur gains two electrons. Sulfur needs two more electrons to achieve the stable electron configuration of the noble gas argon (Ar). The neutral sulfur atom has the electron configuration \[ 1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^4 \]. By adding two electrons, it becomes S虏鈦�, with the configuration \[ 1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^6 \]. These additional electrons fill the 3p sublevel, creating an anion with a -2 charge.
strontium ion
Strontium ion (Sr虏鈦�) forms when strontium loses two electrons to achieve a stable electron configuration similar to krypton (Kr). The neutral strontium atom has the electron configuration \[ 1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^6 \ 4s^2 \ 3d^{10} \ 4p^6 \ 5s^2 \]. By losing two electrons from the 5s orbital, the configuration for Sr虏鈦� becomes \[ 1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^6 \ 4s^2 \ 3d^{10} \ 4p^6 \]. This loss results in a +2 charge commonly observed in group 2 elements.
