Using a periodic table, determine the number of electrons held in energy levels 1-3 of each atom.
B----2 in level 1--3 in level 2--0 in level 3
C--2 in level 1--4 in level 2--0 in level 3
Mg--2 in level 1--8 in level 2--2 in level 3
all ok.
Well, B is like someone with a small house. Level 1 can hold 2 electrons, level 2 can hold 8, but level 3 is empty. So B has 2 electrons in level 1, 3 electrons in level 2, and 0 electrons in level 3.
C is like a slightly bigger house. It also has 2 electrons in level 1, but it has 4 electrons in level 2, and still 0 electrons in level 3.
Mg is like a mansion! It has 2 electrons in level 1, 8 electrons in level 2, and even 2 electrons in level 3. So it's got the most partying going on in level 3.
To determine the number of electrons held in energy levels 1-3 of each atom using a periodic table, you can follow these steps:
1. Locate the atom on the periodic table.
2. Identify the atomic number of the atom. This number represents the number of protons in the atom, which is equal to the number of electrons in a neutral atom.
3. Determine the electron configuration of the atom, which describes how the electrons are distributed among the different energy levels.
Let's go through the atoms you provided:
1. B (Boron)
- Atomic number: 5
- Electron configuration: 1s² 2s² 2p¹
- Electrons in energy levels:
- Level 1: 2 electrons
- Level 2: 3 electrons
- Level 3: 0 electrons
2. C (Carbon)
- Atomic number: 6
- Electron configuration: 1s² 2s² 2p²
- Electrons in energy levels:
- Level 1: 2 electrons
- Level 2: 4 electrons
- Level 3: 0 electrons
3. Mg (Magnesium)
- Atomic number: 12
- Electron configuration: 1s² 2s² 2p⁶ 3s²
- Electrons in energy levels:
- Level 1: 2 electrons
- Level 2: 8 electrons
- Level 3: 2 electrons
Remember that the number of electrons in each energy level is based on the filling order of the orbitals and the maximum number of electrons each level can hold.
To determine the number of electrons held in energy levels 1-3 of each atom using a periodic table, we need to understand the electron configuration of each element. The electron configuration is a representation of how electrons are distributed in energy levels.
For the element B (Boron), the atomic number is 5, meaning it has 5 electrons. The electron configuration for Boron is 1s2 2s2 2p1. This means that 2 electrons are in energy level 1 (1s subshell), 2 electrons are in energy level 2 (2s subshell), and 1 electron is in energy level 2 (2p subshell). Therefore, Boron has 2 electrons in level 1, 3 electrons in level 2, and 0 electrons in level 3.
For the element C (Carbon), the atomic number is 6, meaning it has 6 electrons. The electron configuration for Carbon is 1s2 2s2 2p2. This means that 2 electrons are in energy level 1 (1s subshell), 2 electrons are in energy level 2 (2s subshell), and 2 electrons are in energy level 2 (2p subshell). Therefore, Carbon has 2 electrons in level 1, 4 electrons in level 2, and 0 electrons in level 3.
For the element Mg (Magnesium), the atomic number is 12, meaning it has 12 electrons. The electron configuration for Magnesium is 1s2 2s2 2p6 3s2. This means that 2 electrons are in energy level 1 (1s subshell), 2 electrons are in energy level 2 (2s subshell), 6 electrons are in energy level 2 (2p subshell), and 2 electrons are in energy level 3 (3s subshell). Therefore, Magnesium has 2 electrons in level 1, 8 electrons in level 2, and 2 electrons in level 3.
Using this approach, you can determine the number of electrons held in energy levels 1-3 for any element on the periodic table by analyzing its electron configuration.