3.1: Bonding Theory and Lewis Formulas

Question 1

Define structural formula

Answer 1

a dash between bonding atoms to illustrate the bonds

Question 2

Define valence electrons

Answer 2

electrons in the highest energy level that are being shared by 2 elements in a covalent bond

Question 3

What is a covalent bond

Answer 3

attraction of 2 atoms nuclei for the valence electrons they share

Question 4

Define orbital

Answer 4

specific volume of space where an electron of a certain energy will be found

Question 5

Define valence orbitals

Answer 5

the space where the electrons at the highest energy level occupy

Question 6

Define bonding electron

Answer 6

a valence orbital with only 1 electron, enough space to share electrons with another atom

Question 7

Define lone pair

Answer 7

2 electrons that occupy the valence orbital and have a repelling effect on electrons in any nearby orbital

Question 8

Define Lewis symbol

Answer 8

diagram of an atom with valence electrons drawn as dots around the central symbol, it shows a net charge of zero

Question 9

How does being close to the nucleus affect the electron attraction?

Answer 9

The closer the electron is to the nucleus the more attraction it has towards it so it has less attraction to another electron

Question 10

What do inner electrons shield the nucleus from?

Answer 10

shield the valence electrons from nucleus positive charge

Question 11

What increases the attraction for electrons?

Answer 11

higher amount of protons in the nucleus attract more electrons

Question 12

Define electronegativity

Answer 12

the relative ability of an atom to attract a pair of bonding atoms in its valence level.

Question 13

What element has the highest electronegativity? Which has the lowest?

Answer 13

• Fluorine with a 4.0 (highest)

- Cesium with a 0.8 (lowest)

Question 14

Define covalent bond

Answer 14

simultaneous attraction of 2 nuclei for a shared pair of bonding electrons, in nonmetals (molecular) and it is when electronegativity of both atoms is fairly high

Question 15

What is the “tug-of-war” of bonding electrons?

Answer 15

When atoms collide and the orbitals overlap, each nucleus will fight for the electron pair.

Question 16

Define ionic bond

Answer 16

when the electronegativity is different between colliding atoms and an electron transfer occurs.

Question 17

Define metallic bonding

Answer 17

both colliding atoms have low electronegativity and the atoms can share valence electrons but no chemical reaction takes place. The atoms more around freely with the valence electrons holding everything in place

Question 18

What does metallic bonding allow to happen?

Answer 18

metals can have malleability ductility, flexibility. Because the valence attraction is free to move around and mold into any shape