## What is the energy of energy level 4?

Energy Levels of Electrons

Energy Level Energy
2 -3.4 eV
3 -1.51 eV
4 -.85 eV
5 -.54 eV

## How many electrons can energy level 4?

32 electrons
Thus, the fourth level can hold up to 32 electrons: 2 in the s orbital, 6 in the three p orbitals, 10 in the five d orbitals, and 14 in the seven f orbitals. The sublevels of the first four principal energy levels and the maximum number of electrons that the sublevels can contain are summarized in Table 5.1.

How many electron energy levels are in period 4 elements?

Number of energy levels in each period The atoms in the third period have electrons in 3 energy levels. The atoms in the fourth period have electrons in 4 energy levels.

### What are the first 4 energy levels?

There are four types of orbitals that you should be familiar with s, p, d and f (sharp, principle, diffuse and fundamental). Within each shell of an atom there are some combinations of orbitals.

### How many electrons can you have in the 4th Shell?

This shell can contain a maximum of two electrons. The second shell can hold a maximum of eight electrons. When this is filled, electrons go into the third shell, which also holds a maximum of eight electrons. Then the fourth shell begins to fill….Electron shells.

Energy shell Maximum number of electrons
Second 8
Third 8

Which element has 3 energy levels and 4 valence electrons?

Element Element Number Number of Electrons in each Level
Lithium 3 1
Beryllium 4 2
Boron 5 3
Carbon 6 4

#### Which electrons have the most energy?

Electrons at higher energy levels, which are farther from the nucleus, have more energy. They also have more orbitals and greater possible numbers of electrons. Electrons at the outermost energy level of an atom are called valence electrons.

What is the energy of energy level 4? Energy Levels of Electrons Energy Level Energy 2 -3.4 eV 3 -1.51 eV 4 -.85 eV 5 -.54 eV How many electrons can energy level 4? 32 electrons Thus, the fourth level can hold up to 32 electrons: 2 in the s orbital, 6 in the three…