unit 5 electrons in light

Electrons in energy levels farther from the nucleus have ________ energy than/as electrons in energy levels closer to the nucleus.

• less

• depends on the element

• greater

• the same

Tags

NGSS.HS-PS1-1

There are ___ orbitals in the f sublevel, so the f sublevel can hold ___ electrons.

• 1, 2

• 3, 6

• 5, 10

• 7, 14

"Electrons will fill empty orbitals of the same energy before electrons begin to pair up in the same orbital” best describes which of the following:

• Aufbau Principle

• Hund’s Rule

• Pauli Exclusion Principle

• Heisenberg Uncertainty Principle

"Electrons will fill orbitals requiring lower energy before filling an orbital requiring more energy” best describes which of the following:

• Aufbau Principle

• Hund’s Rule

• Pauli Exclusion Principle

• Heisenberg Uncertainty Principle

Why are we able to use Shorthand Electron Notation?

• only the lowest energy electrons contribute to chemical reactions and properties

• only the highest energy electrons contribute to chemical reactions and properties

• it saves time and space

• noble gasses give a more accurate model of the electron cloud

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

An excited atom is an atom that:

• has at least one electron occupying an energy level above its ground state

• has all of its electrons occupying higher energy levels

• is just excited to be here

• contains enough energy that the atom becomes unstable

How many energy levels are on the periodic table?

• 4

• 5

• 6

• 7

What element ends in: 4d⁸

• Pd

• Pt

• Ni

• Ag

Tags

NGSS.HS-PS1-1

T/F: Electrons fill orbitals one at a time until each has one before they start to double up

• True

• False

How many orbitals (lines/boxes) does the sub level 'p' have?

• 1

• 3

• 5

• 7