Science 5.1-6.2

Front 1

Who was Mendeleev?

Back 1

A Russian chemist and teacher named Dmitri who discovered an organizing principle for all known elements

Front 2

What were Mendeleev's main contributions to science?

Back 2

Mendeleev organized elements based on properties- rows (increasing mass) and columns (similiar properties)

Front 3

Why was Mendeleev's periodic table such a good model?

Back 3

The close match between Mendeleev's predictions and the actual properties of new elements showed how useful his periodic table could be

Front 4

Define Periodic Law

Back 4

The properties of the elements prepeating at regular intervals when the elements are arranged in order of increasing atomic number

Front 5

Define Period/series

Back 5

rows- increasing atomic number

Front 6

Define Group/family

Back 6

columns- properties of elements repeating in predictable ways in a group and have similiar electron configurations

Front 7

What are the modern parts of the periodic table?

Back 7

metals, nonmetals, and metalloids

Front 8

What can you tell about an element from the periodic table?

Back 8

atomic #, name of element, symbol, and atomic mass

Front 9

define metal.

Back 9

elements that are good conductors of electric current and heat

Front 10

Define nonmetal.

Back 10

elements that are poor conductors of heat and electric current

Front 11

Define metalloid.

Back 11

elements with properties that fall between those of metals and nonmetals

Front 12

define valence electron

Back 12

an electron that is in the highest occupied energy level of an atom

Front 13

Why are valence electrons important to the periodic table?

Back 13

because having the same number of valence electrons is why elements in the same group have similiar properties

Front 14

electron configuration

Back 14

the arrangement of electrons in the orbitals of an atom

Front 15

Why is electron configuration important to the periodic table?

Back 15

The number of an A group matches the number of valence electrons in an electron configuration for an element in that group.

Front 16

electron dot diagram

Back 16

a diagram of an atom, ion or molecule in which each dot represents a valence electron

Front 17

why is the electron dot diagram important to the periodic table?

Back 17

because it tells the number of valence electrons

Front 18

Alkali Metals

Back 18

1A

Front 19

Alkaline earth metals

Back 19

2A

Front 20

The Boron Family

Back 20

3A

Front 21

The Carbon Family

Back 21

4A

Front 22

The Nitrogen Family

Back 22

5A

Front 23

The Oxygen Family

Back 23

6A

Front 24

Halogens

Back 24

7A

Front 25

Noble Gases

Back 25

8A- unreactive

Front 26

Transition Elements

Back 26

all elements that do not have groups

Front 27

Inner Transition Elements

Back 27

elements at the bottom of the periodic table- not attached

Front 28

ionic bonding

Back 28

tranferring of an electron or electrons from one atom to another

Front 29

properties of ionic compounds

Back 29

strong attractions among ions within a crystal lattice

Front 30

metals in ionic bonding

Back 30

lose electrons and become positive ions

Front 31

nonmetals in ionic bonding

Back 31

gain electrons and become negative ions

Front 32

How are positive and negative ions arranged in ionic bonding

Back 32

in crystal lattic pattern where each positie ion is surrounded by negative ions and each negative ion is surrounded by positive ions

Front 33

covalent bonding

Back 33

sharing of electrons between two atoms

Front 34

nonmetals in covalent bonding

Back 34

usually C,H,O,N,S,P

Front 35

Molecule

Back 35

basic unit

Front 36

single covalent bonding

Back 36

single pair of electrons are shared Ex.- H:H

Front 37

double covalent bonding

Back 37

2 pairs of electrons are shared Ex.- 0=0

Front 38

triple covalent bonding

Back 38

3 pairs of electrons are shared