Topic 8: Spectroscopy, Video A: Orbital Energies Flashcards Preview

General Chemistry 102 > Topic 8: Spectroscopy, Video A: Orbital Energies > Flashcards

Flashcards in Topic 8: Spectroscopy, Video A: Orbital Energies Deck (14):
1

Neutrons and protons and electrons are located where in the atom?

Neutrons and protons sit in the nucleus while electrons are modeled as dots in orbitals.

2

The 1s orbital represents what energy level?

The 1s orbital represents the n=1 energy level. (The n=1 shell.)

3

What energy level is the 2s and 2p orbital?

n=2 energy level or n=2 shell.

4

When electrons are in their lowest energy levels the atom is said to be in what state?

It's ground state.

5

True or false. All atoms have higher higher energy shells even thought they are unoccupied by electrons.

True.

6

An electron with an energy of 0 is very close or very far from the nucleus?

Very far.

7

In the Rydberg equation what does z equal?

z = the atomic number or the number of protons.

8

In the Rydberg Equation, n equals what?

The shell number or quantum number, also known as the principle quantum number.

9

As you get closer to the nucleus the attractive force gets smaller or larger?

Larger.

10

In the Rydberg equation when n=infinty what does e equal?

0.

11

In the Rydeberg equation when n is very large the energy is very close to what?

The energy is very close to 0.

12

For isoelectronic species the electrons are more tightly bound to the nucleus that has more or less protons?

More protons.

13

When calculating energy, 1 over infinty equals what?

0. By definition.

14

What is the Rydberg equation?

E =-(2.178x10^-18J)z^2/n^2

z=atomic number

n=shell number

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