SI Session 5

An electron transitioned from n = 3 to n = 4. Is this emission or absorption

• absorption

• emission

Tags

NGSS.HS-PS4-3

An electron transitioned from n = 5 to n = 3. Is this emission or absorption?

• emission

• absorption

Tags

NGSS.HS-PS4-3

What is the change in energy associated with the electron transition from n = 5 to n = 6?

• 7.26 x 10^-20

• 7.16 x 10^-20

• 7.20 x 10^-20

• 7.35 x 10^-20

Tags

NGSS.HS-PS3-1

What is the change in energy associated with the electron transition from n = 5 to  n = 1?

• -1.8924 x 10^-18

• -1.624 x 10^-18

• -1.94 x 10^-18

• -1.7424 x 10^-18

Use the de Broglie relationship to determine the wavelength of a 10.0-g ball thrown at a speed of 250 m/s.

• 2.65 x 10^-34 m

• 3.65 x 10^-34 m

• 2.85 x 10^-34 m

• 2.95 x 10^-34 m

Tags

NGSS.HS-PS4-1

Use the de Broglie relationship to determine the wavelength of a lithium atom moving at 2.5 x 10^5 m/s. Mass = 1.15 × 10^-26 kg

• 2.4 * 10 ^-14 m

• 1.3 * 10 ^-14 m

• 2.3 * 10 ^-14 m

• 2.6 * 10 ^-14 m

Tags

NGSS.HS-PS4-1

NGSS.HS-PS4-3

Which of the following quantum numbers determines the shape of an orbital?

• Principal quantum number (n)

• Angular momentum quantum number (l)

• Magnetic quantum number (ml)

• Spin quantum number (ms)

The quantum number Magnetic Quantum Number (ml) determines the

• Orientation of the orbital in space

• Orientation of the orbital in space

• Orientation of the orbital in space

• Orientation of the orbital in space

Which set of quantum numbers is NOT possible for an electron in an atom?

• n=2, l=1, ml​=0, ms=+1/2

• n=4, l=2, ml​=−2, ms=−1/2

• n=1, l=1, ml​=1, ms=+1/2

• n=3, l=2, ml​=1, ms=−1/2

For the quantum numbers n=4, l=3, and ml=1, which type of orbital is the electron in?

• 4d

• 4p

• 3p

• 4f

Tags

NGSS.HS-PS1-1