Question

question 2
1 pts
what is the correct order of increasing electronegativity in the following group of elements?

o c < n < o

o n < c < o

o c < o < n

o o < n < c

question 3
1 pts
which of the following pairs of elements would you expect to form an ionic bond?

o n and p

o c and f

o s and s

o rb and cl

question 4
1 pts
which of the following pairs of elements would you expect to form a polar covalent bond?

o s and s

o b and h

o ba and s

o n and p

Explanation:

Question 2

Electronegativity increases across a period from left to right in the periodic table. Carbon (C), nitrogen (N), and oxygen (O) are in the same period (period 2). As we move from C (group 14) to N (group 15) to O (group 16), the electronegativity increases.

Ionic bonds form between metals and non - metals. Rubidium (Rb) is a metal (alkali metal) and chlorine (Cl) is a non - metal. Nitrogen (N) and phosphorus (P) are both non - metals (form covalent bonds), carbon (C) and fluorine (F) are non - metals (form covalent bonds), and two sulfur (S) atoms will form a non - polar covalent bond (since they are the same element).

A polar covalent bond forms between two non - metals with a significant electronegativity difference. Boron (B) and hydrogen (H) are non - metals. The electronegativity of B is 2.04 and of H is 2.20, creating a small electronegativity difference. Two sulfur (S) atoms form a non - polar covalent bond (same element, no electronegativity difference). Barium (Ba) is a metal and sulfur (S) is a non - metal (form ionic bond). Nitrogen (N) and phosphorus (P) are non - metals but have a relatively small electronegativity difference compared to B - H in this context (N: 3.04, P: 2.19).

Answer:

C < N < O

Question 3