Unit 2 Atomic Theory Part 2 Test Review

Which model of the atom consists of protons and neutrons in a central nucleus, with electrons occupying discrete energy levels surrounding the nucleus?

• Rutherford Model

• Planck Model

• Bohr Model

• Quantum Model

Scientists are consistently building on each other’s models. What did Bohr add to the model of the atom?

• That atoms are solid structures and simple building blocks.

• That atoms have protons and electrons stuck together.

• That atoms have orbiting electrons that can jump energy levels.

• That there is an electron cloud around a nucleus.

In the Bohr model of an atom, protons are represented in blue, the neutrons are red, and the electrons are green. Use your periodic table and determine which of the following atoms is represented by the Bohr model.

• Magnesium

• Calcium

• Aluminum

• Sodium

Tags

NGSS.HS-PS1-1

A group of students was asked to generate statements about the structure of an atom. Which statements accurately describe the structure of atoms? Select TWO correct answers.

• Valence electrons are the electrons located on the outermost energy level.

• Electrons are neutrally charged and located outside the nucleus.

• The nucleus of an atom contains positively charged protons and negatively charged electrons.

• Protons are positively charged and located outside the nucleus.

• The number of neutrons is equal to the mass number minus the number of protons.

Tags

NGSS.MS-PS1-1

Which area of a Bohr Model shows an electron occupying the lowest energy level outside the nucleus of an atom?

• First shell

• Second shell

• Third shell

• Fourth shell

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NGSS.HS-PS1-1

Select which color of visible light has the lowest frequency, and thus, the lowest energy.

• Red

• Orange

• Blue

• Violet

Tags

NGSS.HS-PS4-1

Which of the following waves would have the lowest energy?

• Red wave

• Green wave

• Blue wave

• All three waves have the same energy

Tags

NGSS.HS-PS4-1

NGSS.HS-PS4-4

The bright red line from the emission spectrum of hydrogen has a wavelength of 657nm. What is the energy, in joules, of a single photon of this light?

• 3.03 x 10^{-19} J

• 4.35 x 10^{-40} J

• 3.03 x 10^-28 J

• 4.56 x 10^14 J

Tags

NGSS.HS-PS4-1

A typical cell phone uses wavelengths of 0.36 meters. How much energy does this wave have?

• 2.4 x 10^{-34} J

• 5.5 x 10^-25 J

• 1.1 x 10^{-8} J

• 8.3 x 10^0 J

Tags

NGSS.HS-PS4-1

Red lights on a traffic light have a frequency of 4.3 x 10^14 Hz. What is the red light’s wavelength in meters?

• 1.5 x 10^-49 meters

• 7.0 x 10^{-8} meters

• 1.4 x 10^7 meters

• 1.3 x 10^24 meters

Tags

NGSS.HS-PS4-1