Types of bonding

Question 1

ionic compound

Answer 1

• composed of one metal and one nonmetal

Question 2

What is the empirical formula of the compound with the molecular formula C10H8?

Answer 2

C5H4

Question 3

What is the correct formula for the compound that forms between calcium and sulfur

Answer 3

CaS

Question 4

Name the compound SrI2 and why

Answer 4

• strontium iodide
• Sr is the symbol for strontium, a group 2 element (alkaline earth metal) on the periodic table.
• Metals from group 2 typically form cations with a 2+ charge.
• I₂ represents iodide ions. Iodine (I) is a halogen + tends to gain one electron to form the I⁻ anion, which carries a 1- charge.

Question 5

when do we use roman numerals

Answer 5

• use of Roman numerals, like “(II),” is only necessary when the metal can form more than one type of ion with different charges (oxidation states).

Question 6

when do we use the di prefix

Answer 6

the “di-“ prefix (which means two) is used in naming molecular compounds (compounds between two NON-metals).

Question 7

What is the formula for manganese(IV) oxide?

Answer 7

• One Mn⁴⁺ ion (+4 charge) balances with two O²⁻ ions (each with a 2- charge, so 2 × -2 = -4).
• The sum of the charges (+4 from Mn and -4 from 2 oxygen atoms) equals 0, making the compound neutral.

Question 8

Determine the mass of potassium in 35.5 g of KBr

Answer 8

• The mR mass of KBr = 39.10 g/mol + 79.90 g/mol = 119.00 g/mol.
• 35.5 x 39.10/119 = 11.7

Question 9

moles equation

Answer 9

moles= mass/ molar mass

Question 10

Avogadro’s number (Na)

Answer 10

6.022×10 ^23

Question 11

Numberofmolecules

Answer 11

moles×Na

Question 12

how many electronsn shared in CB

Answer 12

2 electrons

Question 13

When is it appropriate to form double or triple bonds in a Lewis structure

Answer 13

***When the central atom does not have an octet of electron
- Forming a double/triple bond to an atom that already has an expanded octet only adds more electrons around the central atom.
- While oxygen can form double bonds to the central atom, it does not always for a double bond
- Terminal atoms can have lone pairs of electrons without forming a double /triple bond.

Question 14

State the total number of valence electrons in HNO2.

Answer 14

• 18 valence electrons
• H+ has one valence electron (1 atom × 1 electron = 1),
• N3- has five valence electrons (1 atom × 5 electrons = 5),
• O2- has six valence electrons (2 atoms x 6 electrons = 12).