Atom And The Periodic Table

Front 1

A pure substance that cannot be broken down into simpler substances by a chemical reaction

Back 1

Element

Front 2

Each element is identify by_____?

Back 2

One-or two-letter symbol

Front 3

The position of an element in the periodic table tells us much about it _________?

Back 3

Chemical Properties

Front 4

The elements in the periodic table are divided into three groups- ______,________,and ________.

Back 4

Metals

Nonmetals

Mettaloids

Front 5

Identify it's Metals, Nonmetals, and Metalloids

Are located on the left side of the periodic table

Back 5

Metals

Front 6

Identify it's Metals, Nonmetals, and Metalloids

Usually exist as shiny solids

Back 6

Metals

Front 7

Identify it's Metals, Nonmetals, and Metalloids

Are solids at room temperature, except for mercury (Hg), which is a liquid

Back 7

Metals

Front 8

Identify it's Metals, Nonmetals, and Metalloids

Are located on the right side of the periodic table

Back 8

Nonmetals

Front 9

Identify it's Metals, Nonmetals, and Metalloids

Usually do not have a shiny appearance

Back 9

Nonmetals

Front 10

Identify it's Metals, Nonmetals, and Metalloids

Are usually poor conductors of heat and electricity

Back 10

Nonmetals

Front 11

Identify it's Metals, Nonmetals, and Metalloids

Can be solids,liquids, or gasses at room temperature

Back 11

Nonmetals

Front 12

What nonmetals can be solids at room temperature?

Back 12

Sulfur

Carbon

Front 13

What nonmetals can be liquid at room temperature?

Back 13

Bromine

Front 14

What nonmetals can be gasses at room temperature?

Back 14

Nitrogen

Oxygen

Front 15

Identify it's Metals, Nonmetals, and Metalloids

Are located on the solid line that starts at Boron (B) and angles down toward astatine (At)

Back 15

Metalloids

Front 16

Identify it's Metals, Nonmetals, and Metalloids

Have properties intermediate between meals and nonmetals

Back 16

Mettaloids

Front 17

What are the seven mettaloids?

Back 17

Boron

Silicon

Germanium

Arsenic

Antimony

Tellurium

Astatine

Front 18

What are the four elements that make up about 96% of the human body?

Back 18

Carbon

Oxygen

Hydrogen

Nitrogen

Front 19

What is used and stored in large quantities in the body ?

Back 19

Major Minerals

Front 20

Give examples of major minerals.

Back 20

Calcium

Chloride

Magnesium

Phosphorus

Potassium

Sodium

Sulfur

Front 21

What are just as vital to our health as the major minerals, but we don't need large amounts?

Back 21

Trace Minerals

Front 22

Give examples of trace minerals.

Back 22

Iron

Zinc

Boron

Chromium

Iodine

Manganese

Front 23

An element that can be found in hemoglobin, specifically the red blood cells

Back 23

Iron

Front 24

An element that helps the proper functioning of enzymes

Back 24

Zinc

Front 25

An element that functions in your thyroid

Back 25

Iodine

Front 26

A pure substance formed by chemically combining two or more elements together

Back 26

Compound

Front 27

A chemical formula consists of:

Back 27

Element

Subscripts

Front 28

To show the identity of the elements forming a compound

Back 28

Element

Front 29

To show the ratio of atoms in the compound

Back 29

Subscripts

Front 30

Give examples on how compounds can be drawn

Back 30

Ball-and-Stick Representation

Space-Filling Representation

Front 31

All matter is composed of the same basic building blocks called ______?

Back 31

Atoms

Front 32

Atoms are composed of three _________?

Back 32

Sub-atomic Particles

Front 33

-Location of protons and neutrons

-dense core of the atom

-location of most of the atoms mass

Back 33

Nucleus

Front 34

-location of electrons

-compromises most of the atom's volume

Back 34

Electron Cloud

Front 35

Every atom of a given element has the same___________?

Back 35

Atomic Number

Front 36

Every atom of a given element has the same ______________ in the nucleus.

Back 36

Number of protons

Front 37

Different elements have _______ atomic number

Back 37

Different

Front 38

A neutral atom has no net overall charge, so

Z=number of protons= ?

Back 38

Number of electrons

Front 39

Are atoms of the same element that have different number of neutrons

Back 39

Isotopes

Front 40

It is the weighted average of the masses of the naturally occurring isotopes of a particular element in atomic mass unit

Back 40

Atomic Weight

Front 41

What is the atomic weight of chlorine?

Cl-35

Cl-37

Back 41

35.45 amu

Front 42

What medicine can be use to treat thyroid malfunction?

Back 42

Iodine 131

Front 43

What is the row/horizontal in the periodic table is called_____?

Back 43

Period

Front 44

What is the column in the periodic table is called______?

Back 44

Group

Front 45

-Consist of the two columns on the far left and six columns on the far right of the periodic table

- the groups are numbered 1A-BA

Back 45

Main Group Elements

Front 46

-Contained in the 10 short columns in the middle

-these groups are numbered 1B-8B

Back 46

Transition Metal Elements

Front 47

-consist of the lanthanides and actinides

- no group numbers are assigned

Back 47

Inner Transition Elements

Front 48

Elements that compromises a particular group have similar?

Back 48

Chemical Properties

Front 49

Identify if it is Alkali Metals/Alkaline Earth Metals, Halogens, and Noble Gases

Soft and shiny metals

Back 49

Alkali Metals/Alkaline Earth Metals

Front 50

Identify if it is Alkali Metals/Alkaline Earth Metals, Halogens, and Noble Gases

Low melting points

Back 50

Alkali Metals/Alkaline Earth Metals

Front 51

Identify if it is Alkali Metals/Alkaline Earth Metals, Halogens, and Noble Gases

Good conductors of heat and electricity

Back 51

Alkali Metals/Alkaline Earth Metals

Front 52

Identify if it is Alkali Metals/Alkaline Earth Metals, Halogens, and Noble Gases

React with water to form basic solutions

Back 52

Alkali Metals/Alkaline Earth Metals

Front 53

Identify if it is Alkali Metals/Alkaline Earth Metals, Halogens, and Noble Gases

Exist as two atoms joined together

Back 53

Halogens

Front 54

Identify if it is Alkali Metals/Alkaline Earth Metals, Halogens, and Noble Gases

Very reactive; combine with many other elements to form compounds

Back 54

Halogens

Front 55

Identify if it is Alkali Metals/Alkaline Earth Metals, Halogens, and Noble Gases

Very stable

Back 55

Noble gases

Front 56

Identify if it is Alkali Metals/Alkaline Earth Metals, Halogens, and Noble Gases

Rarely combine with any other elements

Back 56

Noble gases

Front 57

Electrons do not move freely in ______?

Back 57

Space

Front 58

An electron is confined to a specific______, giving it a particular energy.

Back 58

Region

Front 59

An electron is confined to a specific______, giving it a particular energy.

Back 59

Region

Front 60

Electrons in lower numbered shells are ______ to nucleus and are _____ in energy.

Back 60

Closer and Lower

Front 61

Electrons in higher numbered shells are ______ from the nucleus and are ____ in energy

Back 61

Further and higher

Front 62

How is the shells being numbered?

Back 62

n= 1,2,3 etc.

Front 63

Shells with larger numbers are further from the nucleus, have a larger ________, and can therefore hold more _______.

Back 63

Volume and electrons

Front 64

Shells are divided into _______?

Back 64

Subshells

Front 65

The subshells are identified by the letters_,_,_,and _?

Back 65

S,P,D and F

Front 66

The subshells consist of the ?

Back 66

Orbitals

Front 67

A region of space where the probability of finding an electron is high.

Back 67

Orbital

Front 68

Each orbital can hold ___ electrons

Back 68

Two

Front 69

The s orbital has a ______ shape

Back 69

Spherical

Front 70

The p orbital has a _______ shape

Back 70

Dumbbell

Front 71

What is the shape of the d orbital?

Back 71

Four leaf clover

Front 72

The __________ describes how the electrons are arranged in an atom's orbital.

Back 72

Electron Configuration

Front 73

The lowest energy arrangement in electron configuration is called the?

Back 73

Ground State

Front 74

Rules in electron configuration

Back 74

1.Electrons are placed in the lowest energy orbital beginning with the 1s orbital.

2. Orbitals are then filled in order of increasing energy

3. Each orbitals hold maximum of 2 electrons

When orbitals are equal in energy:

1 electron is added to each orbital until all of the orbitals are half filled

Then the orbitals can be completely filled

Front 75

An ________ ________ uses a box to represent each orbital and _____ to represent electrons

Back 75

Orbital diagram and arrows

Front 76

The electron configuration can be shortened by:

Back 76

Using the name of the nearest noble gas from the previous rowAdding the en of all remaining electrons

Front 77

The chemical properties of an element depend on the most _____ held electrons, which are found in the ______ ____.

Back 77

Loosely and valence shell

Front 78

The _________ is the outermost shell (highest value)

Back 78

Valence shell

Front 79

The electrons in the valence shell are called ____________ electron.

Back 79

Valence

Front 80

Elements in the same group have similar ________________.

Back 80

Electron Configuration

Front 81

Elements in the same group have the same number of _______________.

Back 81

Valence electrons

Front 82

The groups, _-_, equals the number of valence electrons for the main group elements

Back 82

1A-8A

Front 83

The chemical properties of a group are similar because these elements contain the same ____________ of valence electron

Back 83

Electron configuration

Front 84

_______ representing valence electrons are placed on the four sides of an element

Back 84

Dots

Front 85

Each dot represent ____valence electron

Back 85

One

Front 86

For 1-4 valence electrons, _____dots are used

Back 86

Single

Front 87

With 4 and above valence electrons, the dots are ______?

Back 87

Paired

Front 88

The size of atoms ______ down a column, as the valence e- are farther from the nucleus

Back 88

Increases

Front 89

The size of atoms ______ across a row, as the number of protons in the nucleus increases.

Back 89

Decreases

Front 90

The increasing # of protons pulls the electron closer to the nucleus, making the atoms _______.

Back 90

Smaller

Front 91

The _____________ is the energy needed to remove an electron from a neutral atom.

Back 91

Ionization energy

Front 92

Ionization energies _____ down a column as the valence electrons get father away from the positively charged nucleus

Back 92

Decreases

Front 93

Ionization energies _______ across a row as the number of protons in the nucleus increases

Back 93

Increase

Front 94

What are examples of halogens that can liquid at room temperature?

Back 94

Bromine

Front 95

What are examples of halogens that can solid at room temperature?

Back 95

Iodine

Front 96

What are examples of halogens that can gases at room temperature?

Back 96

Flourine and Chlorine

Front 97

Sodium (Na)

Back 97

Natrium

Front 98

Potassium (K)

Back 98

Kalium

Front 99

Iron (Fe)

Back 99

Ferrum

Front 100

Copper (Cu)

Back 100

Cuprum

Front 101

Silver (Ag)

Back 101

Argentum

Front 102

Tin (Sn)

Back 102

Stannum

Front 103

Antimony (Sb)

Back 103

Stibium

Front 104

Tungsten (w)

Back 104

Wolfram)

Front 105

Gold (Au)

Back 105

Aurum

Front 106

Mercury (Hg)

Back 106

Hydrargyrum

Front 107

Lead (Pb)

Back 107

Plumbum

Front 108

The region occupied by electrons are called _________ energy levels or ____.

Back 108

Principal and shells

Front 109

Two electrons in an orbital have ______ spins, that is ,the spins are opposite in direction, so up and down arrows are used.

Back 109

Paired