Science 9 Chapter 2 Final Exam Review Preparation

Front 1

What are alkali metals?

Back 1

Group 1 metallic elements; all are strongly reactive, soft, low-density metals

Front 2

What are alkaline earth metals?

Back 2

Group 2 elements; all are reactive, soft, low-density metals

Front 3

What is atomic mass?

Back 3

-the mass of an average atom of an element
-usually a decimal number
-measured in amu
-atomic mass and atomic number generally increase with eachother

Front 4

What is the atomic number?

Back 4

the number of protons in each atom of an element

Front 5

What is the Bohr model?

Back 5

a diagram of the atom that describes the arrangement of subatomic particles: neutrons and protons in the nucleus and electrons in electron shells

Front 6

What is a chemical family?

Back 6

groups of elements arranged in vertical columns in the periodic table that have similar physical and chemical properties

Front 7

What are chemical properties?

Back 7

characteristics that describe a substance's ability to react chemically with other substances to form new products

Front 8

What is a chemical symbol?

Back 8

international symbols for each element consisting of one or two letters; the first letter is always capitalized; the second letter is never capitalized

Front 9

What are electron shells?

Back 9

regions surrounding the nucleus of an atom in which electrons move

Front 10

What are halogens?

Back 10

Group 17 non-metallic elements

Front 11

What is an ion?

Back 11

an electrically charged atom

Front 12

What is an ion charge?

Back 12

electrical charge that forms on an atom when it gains or loses electrons

Front 13

What is kinetic energy?

Back 13

energy a moving object has because of its motion; depends on mass and speed of object and the temperature

Front 14

What are metalloids?

Back 14

elements that share some properties with metals and some properties with non-metals

Front 15

What are metals?

Back 15

elements that are typically hard, shiny, malleable, ductile, and good conductors of heat and electricity

Front 16

What is a multiple ion charge?

Back 16

a characteristic of elements that can form ions in more than one way

Front 17

What are non-metals?

Back 17

elements that are typically non-shiny, malleable, or ductile and that are poor conductors of heat and electricity. Non-metals are usually gases or brittle solids at room temperature

Front 18

What is a period?

Back 18

horizontal row in the periodic table

Front 19

What is the periodic table?

Back 19

organized list in which elements are arranged in rows and columns according to their atomic number and their patterns of similar properties

Front 20

What are valence electrons?

Back 20

electrons in the outershell of an atom, which determine its ability to combine with another atom

Front 21

What is the valence shell?

Back 21

the outermost electron shell

Front 22

Who created the periodic table?

Back 22

Dmitri Mendeleev

Front 23

What is the unit for measuring atomic mass?

Back 23

atomic mass unit (amu)

Front 24

What is the pattern for ion forming on the periodic table?

Back 24

Elements on the left side of the periodic table generally form positive; elements on the right except the last column usually form negative ions; elements in the same column will often form ions with the same charge as other elements in that column

Front 25

What are noble gases?

Back 25

Group 18 elements

Front 26

What are characteristics of alkali metals?

Back 26

they are highly reactive, have low melting points and reactivity increases as you go down the column

Front 27

What are characteristics of alkaline earth metals?

Back 27

they are less reactive, and will often burn in the air if heated and react with water (but not as vigorously as alkali metals do)

Front 28

What are characteristics of halogens?

Back 28

they are non-metals and are highly reactive

Front 29

What are characteristics of noble gases?

Back 29

they are the most stable and unreactive elements and are usually odorless and colourless gases at room temperature

Front 30

What are the three patterns in electron arrangements in the periodic table?

Back 30

- most elements in the same family have the same number of valence electrons
- elements in the same period have valence electrons in the same shell
- the period number indicates the number of shells that have electrons

Front 31

Why are noble gases stable?

Back 31

because their valence shells are filled making them stable

Front 32

Why do elements gain or lose electrons?

Back 32

to achieve stability by losing or gaining valence electrons so that they will have the same arrangement as a noble gas in their row on the periodic table

Front 33

How does an atom become an ion?

Back 33

by losing or gaining an electron

Front 34

What are the rules to forming ions?

Back 34

1. an atom of any metal can lose electrons and form positive ions
2. an atom of any non-metal except a noble gas can gain electrons and form negative ions
3. ions have the same electron arrangement as the nearest noble gas

Front 35

How is the charge on an ion show on the symbol of an element?

Back 35

by adding a superscript number followed by a plus or minus sign

Front 36

What is the periodic table?

Back 36

a chart that organizes the elements according to physical and chemical properties

Front 37

How do you calculate the number of neutrons in an element?

Back 37

-atomic mass minus atomic number

Front 38

What are characteristics of atomic numbers?

Back 38

increases left to right in increments of 1

Front 39

What are ion charge patterns?

Back 39

1) elements on the left side of the periodic table tend to form positive ions
2) elements on the right side of the periodic table tend to form negative ions (except for noble gases)
3) elements in the same group often from ions with the same charge

Front 40

Why do patterns in the periodic table occur?

Back 40

a result of regular changes in the structure of atoms of the elements.; elements with similar properties line up in groups, since their electron arrangements are similar

Front 41

What is the rule of the Bohr Model diagram?

Back 41

the 1st shell must be full before the next can be filled etc.

Front 42

What did Bohr propose?

Back 42

-electrons can only travel in fixed orbits around the nucleus
-when electrons move from an outer shell to an inner shell, they emit radiation with a fixed amount of energy

Front 43

The number of elements in each period(row) is...

Back 43

the maximum number of electrons in that electron shell

Front 44

Name the maximum number of electrons that can occupy each shell?

Back 44

1st-2
2nd-8
3rd-8
4th-18

Front 45

What are the valence electron rules?

Back 45

1) elements in same group have the same number of valence electrons (except noble gases)
2) elements in the same period have valence electrons in the same shell
3) period number indicates number of shells that have electrons

Front 46

Name the group and electrons in the valence shell

Back 46

Alkali metals - 1
Alkaline Earth metals - 2
Halogens - 7
Noble gases - 2, 8, 18 (full)

Front 47

What is the stability of metals?

Back 47

often lose electrons from their valence shell to a achieve a stable octet

Front 48

What is the stability of non-metals?

Back 48

often gain enough electrons to achieve the same-arrangement as the noble gas in their row