Physical Science Chapter 18

Front 1

Electron dot structure

Back 1

Shows the valence electrons surrounding the atomic symbol

Electrons placed by themselves, then paired

Front 2

Ionic bond

Back 2

Bond between a metal and non metal (opposite charges)

Net charge is 0, charges balance

Atoms are stable

Front 3

Non bonding pairs

Back 3

Paired valence electrons are stable and rarely form chemical bonds with other atoms

Front 4

Ionic compound

Back 4

All chemical compounds containing ions

Positive and negative charges balance

Brittle like non metals

Front 5

Metallic bond

Back 5

Chemical bond where electrons are shared with all neighbors and hold positively charged metal ions together

Front 6

In a metallic bond, the more electrons that are shared

Back 6

The stronger the bond and the higher the melting point

Front 7

Alloy

Back 7

Any mixture of 2 or more metallic elements

Front 8

Ore

Back 8

Geological deposits containing high concentrations of metal containing compounds

Front 9

Covalent bond

Back 9

Atoms are held together by shared electrons between non metals

Front 10

Covalent compound

Back 10

A substance composed of atoms held together by covalent bonds

Front 11

Molecule

Back 11

Any group of atoms held together by covalent bonds

Front 12

Dipole

Back 12

When the charge in a covalent bond is separated

Front 13

The higher the electronegativity, the higher the

Back 13

Dipole

Front 14

Electronegativity

Back 14

Ability of an atom to pull shared electrons toward itself when bonding

Higher electronegativity, it pulls more

Front 15

Identical atoms have identical

Back 15

Electronegativity

Front 16

Non polar bond

Back 16

When 2 atoms in a covalent bond have the same electronegativity

Front 17

Polar bond

Back 17

Covalent bond between 2 atoms with different electronegativities

Front 18

A dipole is formed when the electronegativity between 2 atoms is greater than

Back 18

.4

Front 19

Nonpolar molecule

Back 19

When dipoles of = strength pull in opposite directions and cancel each other

Front 20

Attraction of molecules

From strongest to weakest

Back 20

Ion-dipole

Dipole-dipole

Dipole- induced-dipole

Induced-dipole - induced-dipole

Front 21

Induced dipole

Back 21

Temporary uneven distribution of electrons

Caused when atoms or molecules get close enough to each other

Front 22

Electron configurations (finding how an element ionizes)

Back 22

Find how many valence electrons

Fewer to add or subtract?

# of added is x-

# subtracted is x+

Front 23

Rules of bonding covalent molecules

Back 23

Duet rule- hydrogen needs 2 electrons

Octet rule- all other atoms need 8 electrons

Front 24

Determining ionic formulas

Back 24

Write down the atoms and how they normally ionize

If they are not neutral, add more until charges balance

Count # needed of each and write formula with suffix of # needed

Front 25

Elements in the same group on the periodic table have the same number of

Back 25

Valence electrons

Front 26

To become a negative ion, does an atom lose or gain electrons?

Back 26

Gain

Front 27

What kind of force holds 2 atoms together within an ionic bond?

Back 27

The electrical force of attraction between oppositely charged ions

Front 28

Elements on _____sides of the periodic table tend to form ionic bonds

Back 28

Opposite

Front 29

Do metals more readily gain or lose electrons?

Back 29

Lose

Front 30

Which elements form covalent bonds?

Back 30

Non metallic elements

Front 31

A dipole is an uneven distribution of ______ in a bond due to the difference in _______ between 2 atoms

Back 31

Electrons

Electronegativity

Front 32

Which element has the greatest electronegativity?

Back 32

Flourine

Front 33

Which element has the least electronegativity?

Back 33

Francium

Front 34

A chemical bond is _____ than the attraction between molecules

Back 34

Bond

Front 35

Induced dipoles are

Back 35

Temporary

Front 36

When an atom loses an electron to another atom this is a

Back 36

Chemical change involving the formation of ions

Front 37

You would have a higher melting point if the charges of ions is

Back 37

Greater

Front 38

Atoms of metallic elements are not good at forming covalent bonds because of their tendency to

Back 38

Lose electrons

Front 39

The further apart on the periodic table, the more

Back 39

Ionic bonds become

Front 40

When Nitrogen and Flourine combine to form a molecule, the chemical formula is

Back 40

NF3

Front 41

Molecules with less symmetry have higher

Back 41

Boiling points

Front 42

Ion-dipole attractions are stronger than dipole-dipole attractions because

Back 42

The magnitude of the electric charge associated with an ion is greater

Front 43

What is a hydrogen bond?

Back 43

An unusually strong dipole-dipole attraction