Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Inorganic Chemistry > Midterm > Flashcards

Midterm Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

What is chemistry

A

Chemistry is the science of the properties structure and transformation of matter.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is matter

A

Matter is anything with mass and takes up space
Matter cannot be destroyed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What’s the law of conservation of mass.

A

Lavoisier (1743-1794)- is a chemical reaction, matter is neither created nor destroyed it is transformed into something else

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Chemical change/ chemical reaction

A

Substances are used up and other compounds are formed to take their place

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Physical change

A

Identity of matter remains the same but involves change in its state

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

States of solids

A

They have a definite shape and a definite volume
All partials are very close together

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

States of liquids

A

Liquids have an indefinite shape and a define volume
Partials are not very close together

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

States of gasses

A

Gasses have an indefinite shape and an indefinite shape
Partials and very far apart and move freely

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Why study the state of matter of a substance

A

To understand how things form/exist
Everything is matter
It’s the building blocks to everything
Risk assessment
Transportation
Handling
Reaction potential

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Physical property states

A

Solid
Liquid
Gas
Plasma

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Physical property change of state

A

Melting
Freezing
Boiling/vaporizing
Condensation
Ionization
Relaxation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Physical property characteristics

A

Colour
Shape
Size
Texture
Mass
Volume
Density

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Chemical property signs of change

A

Order
Change in temp
Change in colour
Bubbles form
Solids form

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Chemical property chemical reactions

A

Atoms from two substances combine to form new substances

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Chemical property examples

A

Burning
Rusting
Rotting
Tarnishing

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What does EC stand for

A

Electrical conductivity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What does DO stand for

A

Dissolved oxygen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Pure substance-element

A

A pure chemical substance consisting of one type of atom which can’t be broken down further
118 elements

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Pure substance-Compound

A

Define and constant composition same properties under a certain set of conditions
Water (H2O) 11.2% by mass H and 88.8% by mass O2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Homogeneous mixture

A

Uniformed composition and properties though the sample
Difficult to see impurities in homogeneous mixture
Ex. Air, gas, salt solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Heterogeneous mixture

A

Non-uniform composition and properties throughout the sample. Different components are visibly distinguishable from one another
Ex. Water and oil

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

How do you test a theory

A

Facts-statement based on direct experiences
Hypothesis-proposed statement to explain facts but lacks proof
Theory- hypothesis with some degree of proof. Establishes a cause and effect relationship

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

How many significant figures is this 4.1658 and 8.45

A

4.1685- 5 significant figures
8.45- 3 significant figures

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Are zeros significant before the decimal

A

No
Ex. 0.004066

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

What BEDMAS

A

Bracket, Exponents, Division, Multiplication, Addition and Subtraction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Addition and subtraction rule

A
  • the final value must have only as many decimal places as the least precise measurement with the least number of decimal places
  • the answer cannot have more digits to the right of the decimal points that any of the original numbers
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Multiply and divide rule

A

-The final value can only have as many significant figures as the least precise measurement with the least number of significant figures
-the number of significant figures in the products or quotient is the determined by the least precise measurement that have the fewest significant figures

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

What is a measurement

A

A method of determining a physical quantity such as length, time and temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Why do we need measurements

A

So we quantify time, distance, plan, schedule, risk, assessment, impacts make decisions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

Quantity of measurements -accuracy

A

-how close a measurement is to the true value
-describes the difference between the measurement and the parts actual value

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Quantity of measurement- precision

A

-how reproducible is the measurement
-describes the variation you see when you measure the same part repeatedly with the same device

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

What three measurement systems are used

A

Metric-world wide- meter, litre, gr, second, Celsius and mol
English system- United States- pounds, inches, gallons and yards
International system of units (SI)- scientific organizations- based on metric system

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

What unit is comparable in all three measurement types

A

Seconds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

What systems use the power of tens for large or very small numbers

A

Metric system and SI

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

Factor label method

A

Set up equation using given units and conversion factor so that the unwanted units cancel remaining desired units

Given x conversion factor=desired

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

Does chemical identity change when substance converts states

A

No

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

What’s the density equation

A

D=m/v

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

Define density

A

Physical property constant at a given temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

Is liquid water denser than solid water

A

Yes- ice represents an open crystal structure of hydrogen bonds. Which is lighter that water due to physical structure.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

Specific gravity equation

A

Density of substance(g/mL)/ density of water (g/mL)
Specific gravity is unit less

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

Application of specific gravity of chemical in the environment

A

Specific gravity>1—> lighter that water= floats

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

Define energy

A

Capacity to do work
2 forms= kinetic and potential

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

What is kinetic energy

A

Energy motion
Possessed by any moving object
Light, heat, mechanical energy
KE=1/2 m. V2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
44
Q

What is potential energy

A

Stored energy
Capacity to move or cause motion due to position
Chemical and nuclear energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
45
Q

Law of conservation of energy

A

Energy can neither be created nor destroyed. It is converted

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
46
Q

Equation for specific heat

A

Q=mc🔺t

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
47
Q

Democritus atom theory

A

Mater is made of very small indestructible units called atoms
He used the word atomos which means not to cut(Greek)
Was the first philosopher to use the word indivisible

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
48
Q

Define elements

A

A substance that consists of the same kind of atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
49
Q

What are the 6 essential elements of living organisms

A

Carbon
Hydrogen
Nitrogen
Oxygen
Phosphorus
Surfer

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
50
Q

Define compound

A

A substance with fixed ratio of elements
Chemical properties differ from elements
20 million known compounds
Characterized by its formula

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
51
Q

Compound formulas-Combining Ratios

A

Formula indicates the atomic symbol of each element and subscript indicates the ratio of an element
HCl

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
52
Q

First postulate of Daltons atomic theory

A

All matter is made up of very tiny indivisible partials called atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
53
Q

Second postulate of Daltons atomic theory

A

All atoms of a given element have the same chemical properties and atoms of different elements have different chemical properties

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
54
Q

Third postulate of Daltons atomic theory

A

In ordinary chemistry reaction No atom of any element can disappear or change into an atom of a different element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
55
Q

Fourth postulate of Daltons atomic theory

A

Compounds are formed by the chemical combination of two or more different kinds of atoms. In a given compound the relative number of each kind of element are constant

56
Q

Fifth postulate of Daltons atomic theory

A

A molecule is a tightly bound combination of two or more atoms that acts as a single unit

57
Q

Law of conservation of mass

A

Total mass of a matter at the beginning and end of an ordinary chemical reaction is the same
Matter can neither be created nor destroyed

58
Q

Law of constant composition

A

The theory Joseph Proust made that support Daltons claims
Any compound is always made up of elements in portion by mass

59
Q

Monoatomic elements

A

Consist of single atoms that are not connected to each other

60
Q

Diatomic elements

A

Two atoms in each molecule connected by a chemical bond O2 ⭕️⭕️
Under normal conditions free atoms don’t exist for these elements

61
Q

Polyatomic element

A

More than two atoms in each molecule connected by chemical bonds
Ex O3 ⭕️⭕️⭕️⭕️

62
Q

What does a atom consist of

A

Protons
Neutrons
Electrons

63
Q

Where are protons and neutrons

A

In the nucleus

64
Q

Where are electrons

A

On the valence rings

65
Q

Define mass number

A

Mass number is one way to describe an atom
It is used to express the relative masses of elements in a compound

66
Q

Define atomic number

A

Number of protons in the nucleus
All atoms of the same element have the same number of protons
118 elements=118 atomic numbers
Neutral atoms: number of electrons= number of protons

67
Q

What are isotopes

A

Isotopes are an element that have the same number of protons but different number of neutrons
Isotopes of an element have almost identical properties except radioactive properties
Protons #= electrons#

68
Q

Do isotopes have the same Z number (atomic number) as # of A (atomic mass)

A

No. Isotopes have the same z but different A

69
Q

Where are isotopes found

A

Most elements are found on earth as mixtures of isotopes most relatively constant ratio

70
Q

What is atomic mass number

A

The mass of a specific isotope
Total mass p+n in an isotope
Measured in amu
= the weighted average of masses of all isotopes
This is given on the period table

71
Q

Predicting relative isotopes abundance

A

Which of the two apropos of antimony is the most abundant in nature: sb-121 (atomic mass 120.9amu) or sb-123 (atomic mass 122.9 amu)
Step 1: look up atomic weight of sb on the periodic table
=121.760 amu
Step 2- compare atomic weight to the isotopes atomic mass see which is closer to the value
Sb-121 120.9amu 121.760-120.9=0.86
Sb-123 122.9amu 122.9-121.760=1.40
Sb in nature is 121.760 amu
Sb-121 is closest to nature
Sb121 =(sb-sb121/ isotopic mass 121-isotopic mass123)x100

72
Q

Calculating % by weight in compounds

A

Step 1-add the molar mass of each element (i) to find the compound molecular weight
Step 2-divid the mass of the element in the compound by the compound’s molecular weight. Multiply by 100% to get percentages

73
Q

Percent abundance of a isotope equation

A

% abundance of isotope=(atomic weight of an element- atomic mass of isotope 2/atomic mass of isotope 1- atomic mass of isotope 2) x100

74
Q

How is a periodic table organized

A

Families or groups=vertical rows
Periods= horizontal rows

75
Q

Main groups of elements

A

1A or iupac 1
2A or iupac 2
3A-8A or iupac 13-18
Transition elements 3B-12B
Inner transition elements 58-71 and 90-103

76
Q

Define metals

A

All but 24 elements are metals
Shiny and ductile
Solids at room temperature
Conduct electricity
Tend to give up electrons
Positive charged

77
Q

Define non metals

A

18 metals
Do not conduct electricity
Solid, liquid or gas at room temperatures
CHNOPS-organic and biochem
Tend to accept electrons

78
Q

Define Metalliods

A

6 elements
Metal and non metal properties

79
Q

Periodicity in the period table

A

Properties vary in regular ways as you move up or down a column
Halogens boiling points increase as you move down
Alkali metals softness increases as you move down

80
Q

Mass and size of an atom

A

Mass of an atom is concentrated in the nucleus (neutrons and electrons are in the nucleus)
Size of an atom is dictated by the electron cloud

81
Q

How to calculate electrons in neutral atoms

A

Number of electrons=number of protons

82
Q

Niels Bohr theory

A

Electron energy is quantized
Ground state=lowest energy level

83
Q

Electron distribution

A

Electrons don’t move freely around the nucleus
Confined to specific regions=principles, energy, levels or shells
Shells are numbered from inside out

84
Q

How many electrons can each leave hold

A

1st level-2 electrons
2nd level-8 electrons
3rd level- 18 electrons
4th level-32 electrons
5th level-50 electrons

85
Q

Possible changes of potential energy in electron distribution

A

An electron can move from one level to another only if the energy gains or loses is exactly equal to the difference in energy between the two levels

86
Q

Describe sub shells

A

Shells are divided into sub shells (s,p,d,f)
Within each shell electrons are grouped into orbital experiments
Each orbital can hold maximum of 2 electrons

87
Q

Define s orbital shapes

A

Sphere shape

88
Q

Define p orbitals shape

A

Dumbbell shape and 90 degrees apart from the centre axis (Px, Py, Pz)

89
Q

Electron configuration of atoms

A

It’s the description of the orbitals that it’s electron occupy
Orbitals available to all atoms are the same regardless of elements
-1s, 2s, 2p, 3s, 3p, ect. ( how they increase)

90
Q

Rule 1 for the ground state configuration

A

Rule 1: orbitals fill in the order of increasing energy from lowest to highest

91
Q

Rule 2 for ground state configuration

A

Each orbital can hold up to two electrons with opposite spins with one arrow pointing up and the other pointing down

92
Q

Rule 3 for ground state configuration

A

Hudes rule: when there is a set of orbitals of equal energy, each orbital becomes half-filled before any are completely filled

93
Q

Showing electron configuration noble gasses

A

Noble gas notation-abbreviated way to show electron configuration of an atom
Uses “previous” noble has to represent all the configuration up to that gas and then show all the subsequent electrons

94
Q

Example of expanded electron configuration

A

Carbon: 1s2,2s2,2px1,2py1

95
Q

Example of condensed electron configuration

A

Carbon 1s2,2s2,2p2

96
Q

Example of noble gas notation electron configuration

A

Carbon (He)2s1,2p2

97
Q

Valence electrons

A

Electrons in the outer most shell of an atom

98
Q

Lewis Dot structure

A

A way represent the valence electrons of an atom with dots around the chemical symbol
Number of dots=number of valence electrons

99
Q

Atomic size and radius

A

Atomic size is determined by the size of its outer most occupied orbit
Atomic radius= atomic mass/ 2

100
Q

Atomic radius-periodic trend

A

Atomic radii (ionic radius) of elements increases Down the groups (columns)
Atomic radii (ionic radius) of elements increases to left across the period (rows)

101
Q

What happens has you go down a group

A

Ionic radius increases
Number of shells increase
More shells of electrons
Shielding increases
Also less attraction means electrons are lulled in less by the nucleus
Atomic radius increases
First ionization energy decreases

102
Q

Ions cations and anions

A

Atoms can gain or lose electrons
Ion= atom with unequal number of protons and electrons
Anion= ion with negative charge
Cation= ion with positive charge

103
Q

Types of cations

A

Formed when electrons are removed from an atom
Positive ions are always smaller then the neutral atom

104
Q

Types of anions

A

Forms when an atom gains electrons
Negative ions are always larger than the neutral atom

105
Q

Ionization energy

A

Ionization energy-a physical property of elements
It is the energy required to remove the most loosely held electron from an atom in the gaseous phase
The more difficult to remove an electron the higher the ionization energy
Ionization energy is always positive because energy must be supplied to remove the attraction force between the nucleus and electrons

106
Q

Ionization energy and periodicity

A

IE increases as you go further up the column (bottom to top)
- electrons further from nucleus are shielded by inner electrons and less attracted to the nucleus therefore less IE is required to remove the outer electrons
IE increases as you go across a row ( left to right)
-valence electrons across a row are in the same shell but number of protons in nucleus increases outer electrons attraction to nucleus and makes them harder to remove

107
Q

Octet rule

A

Lewis observed that the noble gasses lacked chemical reactivity
Thus lack of reactivity indicated a high degree of stability in the noble gas electron configuration
The tendency of atoms to react in different ways to achieve an outer shell configuration of 8 electrons like noble gasses became known as octet rule
Most common among 1A-7A

108
Q

Octet rule ions

A

Atoms with close to 8 valence electrons tend to gain electrons
Gain electrons=negative charge=anions
Atom with 1 or 2 valence electrons tend to lose electrons
Loose electrons=positive charge=cation
Comparing an ion to the original atom #p, and #n are the same only the #e charges in the valence shell

109
Q

First expectation of octet rule

A

Ions of period 1 and 2 with charge greater that +2 are unstable and therefore ions of there elements don’t exist in nature

110
Q

2nd exception to octet rule

A

Octet rule does not apply to group 1B-7B elements (transition elements)
Most of 1B-7B from ions of 2 or more positive charges

111
Q

Properties of atoms and their ions

A

Atoms and their ions have different properties
When Na and Cl are ionized their reactivity decrees and they are stable
When two atoms mix to create an ion it changes their reactivity

112
Q

Naming cations rule 1

A

Elements of groups 1A, 2A and 3A form only one type of cation
The name of the cation is the name of the metal followed by the ions
Ex. Hydrogen ion

113
Q

Naming cations rule 2

A

Two types of cations formed:
Systematic names: use a Roman numeral enclosed in parentheses following the name of the element to show the charge

Older common system: use the suffix-ous to show the smaller positive charge and the suffix -Ic to show larger positive charge

114
Q

Naming anions

A

For monatomic (containing only one atom) anions add ide to the stem name
Ex. Bromide

115
Q

Chemical bonds

A

Atoms born together so that each atom participating in the bond acquires a valence shell electron configuration the same as that of noble gas nearest to it in atomic number

116
Q

Ionic bonds

A

Results from the force of attraction between cations and anions

117
Q

Covalent bonds

A

Results from the force of attraction between 2 atoms sharing one or more pairs of electrons

118
Q

How compounds are formed ( daltons 4th postulate)

A

Compounds are formed when atoms of more that one element combine a given compound always the same relative number and kind of atom
Compounds are tightly bonded groups of atoms held together by forces of attraction called chemical bonds

119
Q

Ionic bond formation

A

Forces of attraction between a cation and anion
One atom donates electors another atom
Generally between metals and non metals
High boiling and melting points
Requires a lot of energy to break ionic bond
Electronegativity difference >1.9

120
Q

Define electronegativity

A

A measure of an atoms attraction for the electrons it shares in a chemical bond with another atoms

121
Q

Ionic compounds

A

Name for the entity formed by electrostatic attraction of positive and negative ions

Elements with higher EN gains electrons
Elements with lower EN donates electrons

122
Q

Rule 1 binary ionic compounds

A

When only one oxidation state: cation name+ stem of anion with the suffix ide

123
Q

Define binary

A

Contains two elements

124
Q

Rule 2 naming binary ionic compounds

A

When >1 oxidation state:cation name+Roman numeral for charge+ stem of anion name with the suffix ide

125
Q

Common naming rule binary ionic compounds

A

When >1 oxidation state:cation Latin root+ous or Ic suffix+ stem of anion name with the suffix ide

126
Q

Naming polyatomic ionic compounds

A

Naming polyatomic ion as a unit
Cation name + anion name

127
Q

Predicting ionic compound formula

A

Strategy: sum of positive charge=sum of negative charge
To product formula simply balance # atoms so cation and anions are equal
Subscripts represent ratios reduced to lowest whole number

128
Q

Ionic compound formula groups and their charges

A

Group 1 ions ( alkali metals) have +1 charges
Group 2 ions (alkaline earth metals) have +2 charges
Group 6 ions (non metals) have -2 charges
Group 7 ions (halogens) have -1 charges

129
Q

Covalent bond formation

A

Force of attraction between 2 atoms sharing one or more pairs of electrons to attain valence electrons configuration of noble gas

130
Q

What are covalent bonds are generally between what?

A

Non metals and non metals
Non metals and metalloids

Lower boiling and melting points require less energy to break down a covalent bond electronegativity less than 1.9

131
Q

Polar covalent bonds

A

EN difference=0.5 to less than 1.9
Unequal sharing of electrons partial charges on atoms

132
Q

Non polar covalent bonds

A

EN difference=less than 0.5
Atoms share electrons equally

133
Q

Electronegativity of noble gasses

A

Noble gasses have No electronegativity
Research showed that relatively stable compounds and both Xe and Kr exist in nature with F, Cl and or O

134
Q

Sigma bonds

A

The orbitals involves in the bond face each other (stronger bond) (single bond/saturated)

135
Q

Pie bonds

A

The orbitals involve in the bonds are parallel to each other ( not as sting as sigma) ( single or triple bonds/ unsaturated)

Inorganic Chemistry (1 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions