chemistry test covalent bonding

Question 1

Explain why a covalent bond forms at the lowest potential energy and how this relates to bond length.

Answer 1

When atoms are at their lowest energy they are at the most stable which is when a bond may be made. The bond length is when attractive when the attractive and repulsive forces are balanced, and potential energy is lowest.

Key: Lowest energy is stable, bond length is about balanced repulsed forces.

Question 2

summarize what you look for in the formula when identifying the following bond types:

-Ionic

Answer 2

A metal and a nonmetal.

Question 3

summarize what you look for in the formula when identifying the following bond types:

-Nonpolar covalent

Answer 3

The electronegativity between atoms is 0. Two nonmetals close on the periodic table.

Question 4

summarize what you look for in the formula when identifying the following bond types:

-Polar Covalent

Answer 4

A slight positive charge or slightly negative charge develops at each pole of the bond. 2 nonmetals further away on the periodic table

Question 5

summarize what you look for in the formula when identifying the following bond types:

-metallic

Answer 5

Metal elements in the equation (at least two).

Question 6

two atoms share electrons unequally.

Answer 6

Polar bond

Question 7

positive nuclei are immersed in a sea of mobile electrons.

Answer 7

metallic Bond

Question 8

Two atoms share electrons equally.

Answer 8

Nonpolar Bond

Question 9

A bond between a metal atom and a nonmetal atom.

Answer 9

Ionic Bond

Question 10

One atom transfers an electron to another atom.

Answer 10

Ionic Bond

Question 11

A bond between different nonmetal atoms.

Answer 11

Polar Bond

Question 12

A bond resulting from electrostatic attractions between opposite charges.

Answer 12

Ionic Bond

Question 13

One atom loses electrons and another atom gains electrons.

Answer 13

Ionic Bond

Question 14

What factor causes some combinations of atoms to form ions, and other combinations of atoms to form covalent bonds.

Answer 14

Electronegativity is the main difference in if it’ll be ionic or covalent, ionic bonds have a large electronegativity difference while covalent bonds have similar electronegativity.

Question 15

What is a nonpolar covalent bond? Explain the electronegativity differences attributed to this type of bond.

Answer 15

A nonpolar covalent is a chemical bond where two atoms share a pair of electrons equally. The electronegativity has similar values between the atoms.

Question 16

What is a polar bond? Explain the electronegativity differences attributed to this type of bond.

Answer 16

A chemical bond where two atoms share a pair of electrons unequally, the electronegativity is much different between the two atoms.

Question 17

Explain the relationship between electronegativity and polarity.

Answer 17

Electronegativity is the attraction between atoms (the pull) and polarity refers to the distribution of electrical charge among the atoms. The relationship between the two is when the electronegativity is a large difference that means it’s a polar molecule.

Large electronegativity = polarity

Question 18

What is a dipole?

Answer 18

A molecule when One end’s side has a slight positive and one side has a slight negative.

Question 19

What symbol indicates a partial charge?

Answer 19

𝛿 +(alpha)

Question 20

How do you determine which atom gets the partial negative charge?

Answer 20

The more electronegative atom is the one with a partial negative charge.

Question 21

indicate which atom will receive the partial negative charge and which atom will receive the partial positive charge.

Answer 21

The more electronegative one gets the neg charge.

Question 22

Explain the difference between a molecule and a formula unit.

Answer 22

Molecules have all of the properties of that substance and can participate in a chemical reaction. It is composed of two or more elements that are covalently bonded together. A formula unit is the smallest electrically neutral collection of cations and anions that compose an ionic compound. (NaCl) is 1 (Na+) and 1 (Cl-).

Question 23

ionic

Answer 23

No sharing of electrons in bond.

It’s a transfer from one to another.

Question 24

nonpolar covalent

Answer 24

Equal sharing of electrons

Question 25

How is the strength of a covalent bond related to its bond dissociation energy?

Answer 25

The dissociation energy is the energy needed to break the bond, so, the stronger the bond the more dissociation energy required.

Question 26

Contrast a sigma bond with a pi bond.

Answer 26

Sigma is direct overlap of atomic orbitals; Pi is side-to-side overlap. Sigma is stronger, has shorter lengths and is less reactive, and has free rotation between bonded atoms.

Question 27

Why can Carbon form 4 bonds even though the orbital notation for carbon suggests only two bonds can form?

Answer 27

When carbon is excited one of the 2s orbital gets upped to the empty 2pz orbital, the 2s and 3 2p orbital combine to form 4 bonds.

Question 28

three lines connecting elements?

Answer 28

1 sigma and 2 pi bonds.

Question 29

two lines connecting elements?

Answer 29

Pi bond.