Chemistry- Chapter 2 Test 1

Front 1

Of the ________ known elements, ______ are naturally occurring and the remaining ______ have been prepared by scientists in the laboratory. Each element is identified by a one- or two letter _________.

Back 1

-118

-90

-28

-Symbol

Front 2

3 different types of elements?

Back 2

-Metals

-Nonmetals

-Metalloids

Front 3

Shiny substances that conduct heat and electricity?

Back 3

Metals

Front 4

Ductile, meaning they can be drawn into wires, and malleable, meaning they can be hammered into shapes?

Back 4

Metals

Front 5

Have properties intermediate between metals and nonmetals?

Back 5

Metalloids

Front 6

Are poor conductors of heat and electricity?

Back 6

Nonmetals

Front 7

All metals are solid at room temp except for __________, which is liquid.

Back 7

Mercury (liquid)

Front 8

Do not have shiny appearance and are poor conductors of heat and electricity?

Back 8

Nonmetals

Front 9

AT ROOM TEMP for NON METALS:

1. Sulfur and Carbon- ____________.

2. Bromine- ____________.

3. Nitrogen, oxygen, 9 other gases- ___________.

Back 9

-Solids

-Liquid

-Gases

Front 10

4 nonmetals that comprise of 96% of the mass of the human body? What are they called?

Back 10

-Oxygen

-Carob

-Hydrogen

-Nitrogen

-Building-block elements

Front 11

3 building-block elements found in the four main types of biological molecules? What are the biological molecules?

Back 11

-Carbon

-Hydrogen

-Oxygen

-Proteins

-Carbohydrates

-Lipids

-Nucleic acids

Front 12

Major minerals are also known as _______________.

Back 12

Macronutrients (potassium, sodium, chlorine, magnesium, sulfur, calcium, phosphorus)

Front 13

Trace elements are also known as _______________ which are required in the daily diet in small quantities usually less than 15 mg.

Back 13

Micronutrients

Front 14

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

Back 14

Compound

Front 15

Uses element symbols to show the identity of the elements forming a compound and subscripts to show the ratio of atoms contained in the compound?

Back 15

Chemical Formula

Front 16

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

Back 16

Atoms

Front 17

Proton, symbolized by ______, has a ______ charge. Electron, symbolized by _____, has a ______ charge. Neutron, symbolized by ______, has ______ charge.

Back 17

-p, +

-e, -

-n, no charge

Front 18

__________ and __________ have approximately the same, exceedingly small mass. The mass of a __________ is much less.

Back 18

-Protons

-Neutrons

-Electron

Front 19

A dense core that contains the protons and neutrons?

Back 19

Nucleus

Front 20

Most of the mass in an atom resides in the ____________.

Back 20

Nucleus

Front 21

Composed of electrons that move rapidly in the almost empty space surrounding the nucleus?

Back 21

Electron Cloud

Front 22

Comprises most of the volume of an atom?

Back 22

Electron Cloud

Front 23

Opposite charges _____________ while like charges _____________.

Back 23

-Attract

-Repel

Front 24

Defines the mass of individual atoms relative to a standard mass?

Back 24

Atomic Mass Unit

Front 25

Every atom of a given type of element always has the _________ number of protons in the nucleus called the __________________.

Back 25

-Same

-Atomic Number (Z)

Front 26

Atomic number = ?

Back 26

-Number of protons in the nucleus= number of electrons

Front 27

Symbolized by A, the sum of the number of protons and neutrons?

Back 27

Mass Number

Front 28

Mass number = ?

Back 28

-number of protons + number of neutrons

Front 29

Two atoms of the same element always have the same number of ____________, but number of ___________ can vary.

Back 29

-Protons

-Neutrons

Front 30

Atoms of the same element having a different number of neutrons?

Back 30

Isotopes

Front 31

An isotope symbol is written using the element symbol with the atomic number as the ________________ and the mass number as the _________________. Both are to the left.

Back 31

-Subscript- A #

-Superscript- M #

Front 32

Hydrogen atoms that have one proton and one neutron, giving them a mass number of 2?

Back 32

Deuterium (D)

Front 33

Hydrogen atoms containing one proton and two neutrons, giving them a mass number of 3?

Back 33

Tritium (T)

Front 34

The weighted average of the mass of the naturally occurring isotopes of a particular element reported in atomic mass units?

Back 34

Atomic Weight (atomic mass)

Front 35

Isotope that emits particles or energy as some form of radiation?

Back 35

Radioactive Isotopes

Front 36

Radioactive Isotopes have both ___________ and ____________ uses in medicine.

Back 36

-Diagnostic

-Therapeutic

Front 37

Row in the periodic table?

Back 37

Period

Front 38

Elements in the same period (row) are similar in?

Back 38

Size

Front 39

Column in the periodic table?

Back 39

Column

Front 40

Elements in the same group (column) have similar?

Back 40

Electronic and Chemical properties

Front 41

Each column in the periodic table is assigned a?

Back 41

Group Number

Front 42

Elements that comprise a particular group have similar?

Back 42

Chemical Properties

Front 43

An Alkali metal group that is soft and shiny and are good conductors of heat and electricity?

Back 43

Alkali Metals

Front 44

An Alkali metal group that have low melting points and react readily with water to form basic solutions?

Back 44

Alkali Metals

Front 45

An Alkali metal group that are shiny solids but less reactive than the other group?

Back 45

Alkali Earth Metals

Front 46

Do the Alkali and Alkali Earth Metals exist in nature as pure elements?

Back 46

NO. THEY ARE ALWAYS COMBINED WITH OTHER ELEMENTS TO FORM COMPOUNDS

Front 47

Very reactive and combine with many other elements to form compounds?

Back 47

Halogens

Front 48

Gases that are especially stable as atoms, and so they are rarely combined with other elements to form compounds?

Back 48

Noble Gases (radon)

Front 49

Hard; Contains a dense three-dimensional network of carbon atoms in six membered rings?

Back 49

Diamond

Front 50

Slippery black substance used as a lubricant; contains parallel sheets of carbon atoms in flat six-membered rings?

Back 50

Graphite

Front 51

Contains 60 carbon atoms joined together in a sphere of 20 hexagons and 12 pentagons in a pattern that resembles a soccer ball or geodesic dome?

Back 51

Buckminsterfullerene (Bucky Ball)

Front 52

___________ ability to join with itself and other elements gives it versatility not seen with any other element in the periodic table?

Back 52

Carbon "party animal of the atomic world"

Front 53

Latches on to many other atoms including itself and holding tight, forming molecular conga lines of hearty robustness- the very trick of nature necessary to build proteins and DNA?

Back 53

Carbon

Front 54

The chemical properties of an element are determined by the number of ____________ in an atom.

Back 54

Electrons

Front 55

Do not move freely in space; rather, it is confined to a specific region, giving it a particular energy?

Back 55

Electrons

Front 56

Occupy discrete energy levels?

Back 56

Electrons

Front 57

It's energy is quantized; that is, the energy is restricted to specific values?

Back 57

Electrons

Front 58

The electrons that surround the nucleus are confined to regions called?

Back 58

Shells (principle energy levels)

Front 59

Shells are numbered 1, 2, 3, 4, and so forth, beginning _________ to the nucleus. Electrons closer to the nucleus are held _________ tightly and have __________ energy. Electrons farther from the nucleus are held _________ tightly and have __________ energy.

Back 59

-Closest

-More

-Lower

-Less

-Higher

Front 60

The farther a shell is from the nucleus, the larger its ______________ becomes, and the ___________ electrons it can hold.

Back 60

-Volume

-More

Front 61

Maximum number electrons that an orbital can hold?

Back 61

2

Front 62

Shells are divided into _____________.

Back 62

Subshells (s, p, d, f)

Front 63

Subshells consist of _____________.

Back 63

Orbitals

Front 64

Region of space where the probability of finding an electron is high?

Back 64

Orbital

Front 65

# OF ORBITALS:

-S=

-P=

-D=

-F=

Back 65

-S= 1

-P=3

-D=5

-F=7

Front 66

Highest to lowest energy level for orbitals?

Back 66

-s, p, d, f

Front 67

Maximum number of orbitals in shell 1?

Back 67

2

Front 68

Maximum number of orbitals in shell 2?

Back 68

8

Front 69

Maximum number of orbitals in shell 3?

Back 69

18

Front 70

Maximum number of orbitals in shell 4?

Back 70

32

Front 71

An s orbital has a _________ of electron density. It is ________ in energy than other orbitals in the same shell because electrons are kept closer to the positively charge nucleus.

Back 71

-Sphere

-Lower

(get larger in size as shell number increases)

Front 72

A p orbital has a ___________ shape. It is ________ in energy than an s orbital in the same shell because its electron density is farther from the nucleus.

Back 72

-Dumbbell

-Higher

(get larger in size as shell number increases)

Front 73

How electrons are arranged in an atom's orbital?

Back 73

Electron configuration

Front 74

The lowest energy arrangement of electrons is called?

Back 74

Ground State

Front 75

Orbital energies increase within a shell in what order?

Back 75

s, p, d, f

Front 76

Uses a box to represent each orbital and arrows to represent electrons?

Back 76

Orbital Diagram

Front 77

A single electron, which is shown by one single arrow pointing up?

Back 77

Unpaired electrons

Front 78

Two electrons in an orbital, that have _______________- (opposite direction) so an up and down arrow are used?

Back 78

Paired Spins

Front 79

_______________ tells us how many electrons must be placed in orbitals.

Back 79

Atomic Number

Front 80

Electrons are always added to the ____________ energy orbitals first.

Back 80

Lowest

Front 81

4 regions that the periodic table can be divided into?

Back 81

Blocks s, p, d, f

Front 82

Blocks are labeled according to the subshells taht are filled with electrons ___________.

Back 82

Last

Front 83

The chemical properties of an element depend on the most loosely held electrons, that is the electrons in the outermost shell, called?

Back 83

Valence Electrons

Front 84

The ___________ number tells the number of valence electrons. To identify electrons in the valence shell, always look for the shell with the ____________ number.

Back 84

-Period

-Highest

Front 85

Elements in the same group have ____________ number of valence electrons and ____________ electronic configuration.

Back 85

-The same

-Similar

Front 86

________________ in a group are similar because these elements contain the same electronic configuration of valence electrons.

Back 86

Chemical properties

Front 87

The periodic table is organized into groups of elements with similar _________________ in the same column.

Back 87

Valence electronic configurations

Front 88

The number of valence electrons around an atom is often represented by?

Back 88

Electron-dot symbol

Front 89

Electron dot symbol: each dot represents 1 ___________________. The dots are placed on the four sides of an element symbol. More than four electrons, the dots are ___________. Location doesn't matter.

Back 89

-Valence electrons

-Paired

Front 90

Properties of an atom that change in a regular way across a row or down a column of a periodic table?

Back 90

Periodic Trends

Front 91

The distance from the nucleus to the outer edge of the valence shell?

Back 91

Atomic radius

Front 92

The size of atoms ______________ down a column of the periodic table, as the valence electrons are farther from the nucleus.

Back 92

Increases

Front 93

The size of atoms _____________ across a row of the periodic table as the number of protons in the nucleus increases. An increasing number of protons pulls the electrons closer to the nucleus, so the atom gets ____________.

Back 93

-Decreases

-Smaller

Front 94

________________ decreases across a row of the periodic table as the number of protons in the nucleus increases.

Back 94

Atomic Radius (size)

Front 95

The more tightly the electron is held, the _________ the energy required to remove it. Removing an electron from a neutral atom forms a __________.

Back 95

-Greater

-Cation

Front 96

Energy needed to remove an electron from a neutral atom?

Back 96

Ionization Energy

Front 97

Positively charged, and has fewer electrons than the neutral atom?

Back 97

Cation

Front 98

Ionization energies __________ down a column of the periodic table as the valence electrons get farther from the positively charged nucleus.

Back 98

Decreases

Front 99

Ionization energies generally ____________ across a row of the periodic table as the number of protons in the nucleus increases.

Back 99

Increases