What is Ionization Energy?

• The energy required to remove an electron from an atom in its gaseous state

• The energy released when an electron is added to an atom

• The energy required to break a chemical bond

• The energy required to change the state of a substance

Tags

NGSS.HS-PS1-2

Electronegativity is defined as:

• The ability of an atom to attract electrons towards itself

• The energy required to remove an electron from an atom

• The energy change when an electron is added to an atom

• The size of an atom

What is the definition of Atomic Radius?

• The distance from the nucleus to the outermost electron

• The number of protons in an atom

• The energy required to remove an electron

• The number of neutrons in an atom

Tags

NGSS.HS-PS1-1

Which of the following scientists used the cathode ray tube experiment to discover the electron and proposed the plum pudding model of the atom?

• Thomson

• Rutherford

What does Rutherford’s Experiment demonstrate about the structure of the atom?

• The atom is a solid sphere.

• The atom has a dense nucleus with electrons orbiting around it.

• The atom is a plum pudding model.

• The atom is indivisible.

Tags

NGSS.HS-PS1-8

Label the following parts of the atom.

What is the relationship between wavelength and frequency? Describe the relationship using the table below.

• As wavelength increases, frequency decreases.
• As wavelength increases, frequency increases

• As wavelength decreases, frequency decreases

• What is wavelength & frequency?

Tags

NGSS.HS-PS4-1

What happens to frequency when wavelength increases?

• Frequency decreases.
• Frequency increases

• Frequency stays the same

• Frequency isn't involved

Tags

NGSS.HS-PS4-1

What happens to frequency when wavelength decreases?

• Frequency increases.
• Frequency decreases

• Frequency stays the same

• Frequency is equal to the wavelength

Tags

NGSS.HS-PS4-1

What is the maximum amount of electrons that can fit in each orbital shape? s orbital: _______ electrons

• 2
• 4

• 6

• 8