Question

16. 15. 14. 12. 13. a. b. C. d. 11 b. C. 9 d. 10 a. 10 a. b. a. C. d. b. C. d. a. b. 6 C. 7 d. 8 If the 2nd a. 5 b. 7 C. d. a. b. C. a. b. d. What is the correct electron configuration for the element: fluorine (F) 1s 2s 3p 1s 2s 3p What is the maximum number of electrons the /orbital can hold? 8 10 12 14 What is the correct arrow notation for nitrogen (N)? 1s 2s (7) (4) (71) (††) 2p (D) (D (D) (†) ( ) ( ) (1) (†) ( ) (TD) (D) (74) (†) (†) ( ) ( ) How many energy levels are there? 5 What is the reason the protons do not collide with each other? The protons do contact each other Electrons form a shield around the nucleus Neutrons form a shield around the nucleus The protons are too small to contact each other 3s (†) ( ) ( ) ( ) What happens when we heat up substances? Electrons increase in energy level which causes light to be produced The electrons go into an excited state followed by a release in energy to the ground state which produces static What is the charge of an electron? Positive Neutral Negative C. d. None of the above 3p ( ) ( ) ( ) ()( )( ) (0) (00) electricity Electrons jump to a new orbital that causes light to be produced The electrons go into an excited state followed by a release in energy to the ground state to produce light energy level has 1 less electron than full, how many electrons are in the atom?​

Answer 1

The correct electron configuration for fluorine (F) is 1s² 2s² 2p⁵. A p orbital can hold a maximum of six electrons. The arrow notation for nitrogen shows one electron in each of the three 2p orbitals, following Hund's rule.

Step-by-step explanation:

The correct electron configuration for the element fluorine (F) is 1s² 2s² 2p⁵. Fluorine has nine electrons, and according to quantum theory, these electrons are distributed over different energy levels and sublevels. The first two electrons fill the 1s sublevel, the next two occupy the 2s sublevel, and the remaining five electrons are assigned to the 2p sublevel.

Regarding the maximum number of electrons that a p orbital can hold, the answer is six. Each p sublevel consists of three orbitals, and since each orbital can hold two electrons with opposite spins, the p sublevel can accommodate a total of six electrons.

For nitrogen (atomic number 7), the arrow notation that depicts its electron configuration would be as follows: 1s (††) 2s (††) 2p (†)(†)(†). This reflects that nitrogen has a fully filled 1s and 2s subshells, with one electron in each of the three 2p orbitals, adhering to Hund's rule of maximum multiplicity.