Lewis Dot and Bohr Models

Describe the element with 2 electrons in the first energy level and 7 electrons in the second energy level.

• It has 9 protons and 9 neutrons in the nucleus.

• It has 8 protons and 8 neutrons in the nucleus.

• It has 10 protons and 10 neutrons in the nucleus.

• It has 7 protons and 7 neutrons in the nucleus.

How many energy levels does a sodium atom have?

• 1 energy level

• 2 energy levels

• 3 energy levels

• 4 energy levels

How many valence electrons does Carbon have?

• 2

• 4

• 6

• 8

What is the shape of the p orbital?

• Spherical

• Dumbbell-shaped

• Cylindrical

• Triangular

What is the significance of valence electrons?

• They determine an element's atomic mass.

• They determine an element's chemical properties and reactivity.

• They are responsible for the color of the element.

• They indicate the number of neutrons in an atom.

Is this the correct dot diagram for sodium (Na)?

• True

• False

• Not enough information

• Only in certain conditions

What can be expected from elements with the same valence electron configuration?

• Similar chemical reactivity

• Different physical properties

• Higher atomic mass

• Increased electronegativity

What is the relationship between atomic number and the number of electrons in a neutral atom?

• In a neutral atom, the number of electrons is greater than the atomic number.

• In a neutral atom, the number of electrons equals the number of protons, which is the atomic number.

• In a neutral atom, the number of electrons is less than the atomic number.

• In a neutral atom, the number of electrons is unrelated to the atomic number.

How do you determine the number of protons in an atom?

• The number of protons is equal to the atomic number of the element.

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

• The number of protons is equal to the mass number of the element.

• The number of protons is equal to the number of electrons in a neutral atom.

What is the electron configuration for Carbon?

• 1s² 2s² 2p²

• 1s² 2s² 2p⁶

• 1s² 2s² 2p¹

• 1s² 2s² 3p²