Bonding Test

Question 2

what is chemical bonding?

Answer 2

how atoms come together

Question 3

Why do atoms bond

Answer 3

-they bond to become stable (most stable when their s and p orbitals of their outer level are full)
-this is called a full octet because it puts 8 in the outer energy level (octet rule)

Question 4

Ionic bond

Answer 4

-electrons are transferred
-formed between a metal and an nm
-smallest units are called formula unit
- cation (looses and e) anion (gains e)
-bond is a mutual attraction between a cation and an anion

Question 5

Monatomic Ions

Answer 5

-ion made of one atom that has lost or gained e’s

Question 6

How to name cations

Answer 6

To name a cation (positive), name the element.
sodium atom (Na) —> sodium ion (Na1+)

Question 7

How to name an anion

Answer 7

To name an anion (negative), replace the ending of the element with -ide and then say ion after

Question 8

Covalent Bonds

Answer 8

electrons are shared
- The smallest unit is a molecule
-formed between 2 or more non-metals or semimetals
-made by sharing valence e-‘s
-the nucleus of one atom attracts the electron cloud of another atom

Question 9

What happens when covalent bonds dissolve

Answer 9

breaks into molecules

Question 10

What happens when ionic bonds dissolve

Answer 10

breaks into atoms

Question 11

Diatomic Molecule (list of them)

Answer 11

HINClBrOF
-two atoms of the same element that are covalently bonded

Question 12

Ionic v.s. Covalent properties (ionic)

Answer 12

-ionic compounds are usually solids and have high melting points and boiling points.
(why?) when melting or dissolving ionic compounds, you are breaking the ionic bond (electrostatic forces).

Question 13

Ionic v.s Covalent properties (covalent)

Answer 13

-are usually liquids and gasses and have lower melting and boiling points
(why?) when melting or dissolving molecular compounds, you are separating individual molecules, not breaking molecular bonds.

Question 14

what kind of bond will it make

Answer 14

bonding is not purely ionic
-the difference in electronegativity determines the nature of a bond

Question 15

large difference in electronegativity

Answer 15

will form an ionic bond

Question 16

small difference in electronegativity

Answer 16

polar covalent bond

Question 17

no difference in electronegativity

Answer 17

non-polar or purely covalent bond

Question 18

The general rule of bonding

Answer 18

metal+nonmental=ionic
nonmetal+nonmetal=polar cov.
2 same nonmetal non-polar cov.

Question 19

Polar molecules

Answer 19

the molecule in which electrons are unequally distributed

Question 20

Metallic Bonding

Answer 20

-within a metal there a no molecules
-metals are bound in crystal structure where every atom is surrounded by the same atoms
-Electrons are delocalized: free to move around the metal. This is called a “sea of electrons”

Question 21

sea of electrons properties

Answer 21

electrical and heat conductivity
malleability
ductility
luster (shininess)

Question 22

Electron Dot Figure

Answer 22

-Only valence electrons are shown
-Dots placed around the element’s symbol
-Cannot have more than 8 dots

Question 23

Double Bond

Answer 23

sharing 2 electron pairs

Question 24

Triple bond

Answer 24

sharing 3 electron pairs

Question 25

what is the bond length

Answer 25

it is the distance between 2 bonded atoms at their minimum potential energy

-the average distance between the nuclei of two atoms that are chemically bonded together in a molecule

Question 26

ionic v.s covalent bond length

Answer 26

in general, ionic bonds are stronger and therefore have a shorter bond length than covalent bonds.

Question 27

bond length (order)

Answer 27

single>double>triple>ionic

Question 28

bond strength

Answer 28

ionic>triple>double>single

Question 29

Polyatomic ions

Answer 29

-certain atoms bond covalently with each other but are charged as a group. these are called polyatomic ion
-when p. ions bond with another ion it makes an ionic bond

Question 30

To do lewis structures (+)

Answer 30

when positively charged subtract e-‘s

Question 31

To do lewis structures (-)

Answer 31

when negatively charged add e-‘s

Question 32

Resonance Structures

Answer 32

set of 2 or more Lewis structures that collectively describe bonding

Question 33

Vesper theory

Answer 33

column 1 is non-polar (only have to do rows 1 2 and 3)

Question 34

properties of ionic compounds

Answer 34

-Ionic compounds are called salts.
-They are brittle solids
Many ionic compounds dissolve in water
-Solutions with dissolved ionic
compounds are electrical
conductors (electrolytes)
-High melting/boiling points