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CHEMISTRY Flashcards

1
Q

Is the study of matter, its proerties, how and why substances combine or separate to form other substances, and how substances interact with energy

A

Chemistry

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2
Q

Branches of Chemistry (5)

Deals with the separation, identification and quantification of chemical substances (analytes) in a gicven sample

A

Analytical chemistry

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3
Q

Branches of Chemistry (5)

Studies the physical properties of chemical compounds using laws and concepts of physics, such as motion, energy, force, time, thermodynamics, quantum chemistry, statistical mechanics and dynamics

A

Physical Chemistry

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4
Q

Branches of Chemistry (5)

Studies the structure, composition, and chemical reactions of chemical components of living systems (plants, insects, viruses, microoragnisms, and mammals) to understand how and why chemical reaction occur in them.

A

Biochemistry

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5
Q

Measurements in Chemistry

123

Identify how many sig figs in example above

A

3 sig figs

Rule: All non-zero digits are significant figures

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6
Q

Measurements in Chemistry

12.507

Identify how many sig figs in example above

A

5 sig figs

Rule: Zeroes between non-zero digits are significant

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7
Q

Measurements in Chemistry

1.02

Identify how many sig figs in example above

A

3 sig figs

Rule: Zeroes between non-zero digits (decimal) are significant

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8
Q

Measurements in Chemistry

0.012

Identify how many sig figs in example above

A

2 sig figs

Rule: Zeroes to the left of the first non-zero digits are not significan

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9
Q

Measurements in Chemistry

2.00

Identify how many sig figs in example above

A

3 sig figs

Rule: Zeroes to the right os decimal point are significant

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10
Q

Measurements in Chemistry

0.012

Identify how many sig figs in example above

A

2 sig figs

Rule: Zeroes to the left of the first non-zero digits are not significan

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11
Q

This refers to the closeness of a measured value to a standard or known value

A

Accuracy

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12
Q

This refers to closeness of two or more measurements to each other aka repeatability

A

Precision

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13
Q

Is anything that occupies physical space and has mass and inertia

A

Matter

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14
Q

What are the 2 kinds of Matter?

A

Pure substance and Mixture

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15
Q

2 kinds of matter

Has contant composition and properties are constant throughout the sample (one set of properties)

ex. melting point, color, boiling point

A

Pure substance

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16
Q

2 kinds of matter

Combination of two or more substances that are not chemically united and do not exist in fixed proportions to each other

ex. most natural substances

A

Mixtures

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17
Q

2 kinds of matter:

2 Types of Pure Substances

A

Elements and Compounds

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18
Q

2 Types of Pure Substances

Substance made up of two or more different elemnts that are joined together in a fixed ratio

A

Compound

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19
Q

2 Types of Pure Substances: Compound

3 types of compounds

A
  1. Ionic compounds
  2. Covalent Compounds
  3. Covalent Network Substances
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20
Q

3 types of compounds

Are compounds composed of disscrete ions or charged species

A

Ionic compounds

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21
Q

3 types of compounds: Ionic Compound

Familiarize the properties of ionic compounds

2 Types of Pure Substances

A
  1. Solid
  2. High melting and boiling points
  3. Soluble in polar liquids like water (not in nonpolar)
  4. Hard
  5. Very reactive
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22
Q

3 types of compounds

Molecule formed by covalent bonds

A

Covalent compound

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23
Q

Bonds

Type of bond which atoms share one or more pairs of valence electrons

A

Covalent bond

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24
Q

3 types of compounds

Familiarize the properties of Covalent Compound

A
  1. High volatility
  2. Weak bonds
  3. Insoluble in water/polar liequids
  4. Low melting point
  5. Form a molecule
  6. Form between two nonmetals
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25
Q

3 types of compounds

Consists of a network of atoms of the same or different elemnts connected to each other by covalent bonds.

Network of these bonds extends throughout crystalline structure

One of the hardest materials on earth

Havehigh melting points and poor conductivity

A

Covalent Network Substances

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26
Q
A
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27
Q

3 types of compounds: Covalent Network Substances

Familiarize the properties of Covalent Network Substances

A
  1. High melting point
  2. Very hard
  3. Non conducting
  4. Insoluble in any solvent
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28
Q

What are the 2 major properties of matter?

A
  1. Physical properties
  2. Chemical properties
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29
Q

What are the 2 properties under physical properties?

A
  1. Intensive property
  2. Extensive property
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30
Q

2 major properties of matter

Can be observed or measured without changing the composition of matter

A

Physical Property

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31
Q
A
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32
Q

2 major properties of matter

Decribe the characteristic ability of a substance to react to form new substances

Flammability, Susceptibility to corrosion

A

Chemical Property

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33
Q

2 properties under Physical Property

A physical property that will be the same regardless of the amount of matter

A

Intensive Property (density, color, luster, odor, malleability, conductivity, hardness, ductility, boiling point, melting point)

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34
Q

2 properties under Physical Property

A physical property that will change if the amount of matter changes

A

Extensive property

MASS, VOLUME, WEIGHT (M V W)

MEMORIZEEEE

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35
Q

2 kinds of changes in matter

A
  1. Physical Change
  2. Chemical Change
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36
Q

2 kinds of changes in matter

Occurs when a substance or object changes its appearance, phase, or is used in a miaxture

Molecular strufcture does not change

A

Physical change

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37
Q

2 kinds of changes in matter: Physical Change

Types of Physical Changes

A
  1. Sublimation
  2. Melting
  3. Freezing
  4. Boiling/Evaporation
  5. Condensation
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38
Q

2 kinds of changes in matter: Types of Physical Change

Solid to Gas:
Liquid to Gas:
Gas to Liquid
Solid to Liquid:
Liquid to solid

Answer the appropriate types of physical changes being described

A

Solid to Gas: Sublimation
Liquid to Gas: Boiling or Evaporation
Gas to Liquid: Condensation
Solid to Liquid: Melting
Liquid to Solid: Freezing

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39
Q

2 kinds of changes in matter

Occurs when the substance’s composition is changed

When bonds are broken and new ones are formed when this change occurs

A

Chemical Change

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40
Q

2 kinds of changes in matter: Chemical change

Types of Chemical Changes

A
  1. Combination/synthesis
  2. Decomposition
  3. Substitution/siNGLE Replacement
  4. Double Discplacement
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41
Q

Types of Chemical Changes

Two or more reactants unite to form a single product

A

Combination or Synthesis

2Na(s) + Cl2(g) → 2NaCl(s)

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42
Q

Types of Chemical Changes

A single reactant is broken down into two or more products

opposite reaction of combination

A

Decomposition

2HgO(s) → 2Hg(l) + O2(g)

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43
Q
A
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44
Q

Types of Chemical Changes

A single free element replaces or is** substituted** for one of the elements in a compound

A

Substitution or Single Replacement

Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g)

Cl2 is substituted / the free element

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45
Q

Types of Chemical Changes

For ionic compounds, the positive ion in the 1st compound combines with the negative ions in the 2nd compound, and the negative ion in the 1st compound combines with the positive ion in the 2nd compound

BASICALLY:
1st compound (+) ion + 2nd compound (-) ion

2nd compound (-) ion + 1st compound (+)

Opposite charges

A

Double displacement reaction

AgNO3 + NaCl → AgCl + NaNO

Exchange of partners yuck

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46
Q

What are the 2 types of mixtures

A
  1. Homogenous
  2. HETERogeneous
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47
Q

2 types of mixtures

Two or more substances that form the mixture are evely distributed througout the mixture

Ex. Vinegar (ethanoic acid + water)

A

Homogenous mixture

bading

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48
Q

2 types of mixtures

Two or more substances that form the mixture are not evenly distributed throughout the mixture

Ex. water and oil

TUBIG AT LANGISSSSSSSS~~~ iykyk

A

Heterogenous mixtures

straight ka aw

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49
Q

Mixture:

Familiarize the Solubility rules

A

Soluble:
1. Alkali metals (Group IA)
2. Ammonium (MH4) copumds
3. Nitrates, Chlorates, Perchlorates (NO3, ClO3, ClO4)
4. Alkali metal Hydroxides; BaOH, CaOH (B, C are only slightly soluble)
5. Chlorides, Bromides, Iodides
6. Most sulfates (SO4),
7. Calcium, Silver (CaSo4, Ag2SO4)

Insoluble:
1. Most Hydroxides (except those mentioned above)
2. Carbonates, Phosphates, Sulfides
3. Barium, Mercury, Lead (BaSO4, HgSO4, PbSO4)

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50
Q

What are the following 3 Laws of Chemical Combination

A
  1. Law of Conservation of Mass
  2. Law of Definite Proportion or Composition
  3. Law of Multiple Proportion
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51
Q

3 Laws of Chemical Combination

States that matter cannot be created or destroyed in a chemical reaction

A

Law of Conservation of Mass

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52
Q
A
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53
Q

3 Laws of Chemical Combination

States that chemical compounds are formed of constant and defined ratios of elements as determined by mass

A

Law of Definite Proportion or Composition

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54
Q
A
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55
Q

3 Laws of Chemical Combination

States that when elements form compounds, the proportions of the elements in those chemical compounds can be expressed in small whole number ratios

A

Law of Multiple Proportion

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56
Q

What are the 5 Major Atomic Theories?

A
  1. John Dalton’s Atomic theory
  2. Thomson’s Plum Pudding Model
  3. Rutherford’s Nuclear Atom Model
  4. Bohr’s Solar System Model of the Atom
  5. Quantum of Wave-Mechanical Model
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57
Q

Identify whivh of the 5 Major Atomic Theories

→ Matter is composed of extremely small particles called atoms that participate in chemical change

→ Element consist only of one atom

→ Atoms of one element differ from atoms from other element

→ Compound consists of atoms of two or more elements combined; always present in constant/fixed ratio

→ Atoms are neither created or destroted, but is rearranged to yield different substances from those in the reactant

A

John Dalton’s Atomic Theory

REMINDER: JD’s theory focused on the definition/properties of an atom, element, compound

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58
Q

Identify whivh of the 5 Major Atomic Theories

→ Matter is composed of extremely small particles called atoms that participate in chemical change

→ Electrons are negatively-charged particles, while Atoms are neutrally-charged

→ Atom consists of a sphere of positive matter within which electrostatic forces determine positioning of the negatively charged cporpuscles (explains the neutral charge of the whole atom)

→ These negatively charged corpuscles were evely distributed in uniform sea of positive charge, like plums in pudding

A

Thompson’s Plum Pudding Model

REMINDER: Bits of (-) charged corpuscles are within scattered (+) charged ions;

UHM search itsura of plum pudding
Plum: (-) charged corpuscles
Pudding: (+) charged ions

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59
Q

Identify whivh of the 5 Major Atomic Theories

→ Was tested by bombarding a thin of sheet of gold with a-particles abd studies the trajectory of particles after interaction with gold foil

→ Most alpha particles passed straight through the foil, indicating that atoms are mostly empty space.

→ However, a small fraction of particles were deflected at large angles (the electron orbit)

→ some even bounced back toward the source (the** nucleus**/mismong gitna which is positive charged)

A

Rutherford’s Nuclear Atom Model (Alpha scattering Experiment)

REMINDER: Mainly stated the existence of (+) charged nucleus and orbit of (-) charged

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60
Q

Identify whivh of the 5 Major Atomic Theories

→ The positively charged particles and most of mass of an atom was concentrated in an extremely small volume called nucleus

→ Negatively charged electrons surround the nucleus and that these electrons surrounding nucleus revolve around it with very high speed in circular paths called orbits

A

Rutherford’s Nuclear Atom Model (Alpha scattering Experiment)

REMINDER: Mainly stated the existence of (+) charged nucleus and **orbit **of (-) charged

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61
Q

Identify whivh of the 5 Major Atomic Theories

→ Electrons only assume only certain orbits around nucleus called stationary orbits

→ Each orbit has an **energy **associated with it (Ex. orbit close to nucleus is E1)

→ Light is **emmited **when electron jumps from higher to lower orbit (nauubusan eh); absorbed when jumps from lower to higher (nadadagdagan)

→ Energy and Frequency of light emitted or absorbed is given by the difference between 2 orbit energies

A

Bohr’s Solar System Model of the Atom

REMINDER: Stated the positioning of electrons, energy of orbit, Light/Energy is emitted or absorbed

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62
Q

Identify whivh of the 5 Major Atomic Theories

→ Electrons are not in Circular orbits around the nucleus

→ Electrons are in a 3-D region around the nucleus called atomic orbitals

→ The atomic orbital describes the probable location of the electron

A

Quantum or Wave-Mechanical Model

REMINDER: Stated that elrctrons are in 3d region/wave??

63
Q

5 Major Atomic Theories: Parts of the Quatum/Wave-Mechanical Model

Highest point of the wave

A

Crest

64
Q

5 Major Atomic Theories: Parts of the Quatum/Wave-Mechanical Model

Lowest point of the wave

A

Trough

65
Q

5 Major Atomic Theories: Parts of the Quatum/Wave-Mechanical Model

Distance from one crest and trough to the next

A

Wavelength

66
Q

5 Major Atomic Theories: Parts of the Quatum/Wave-Mechanical Model

Height from trough to crest

A

Wave Height

67
Q

5 Major Atomic Theories: Parts of the Quatum/Wave-Mechanical Model

Ratio of wave height to wavelength

A

Wave steepness

68
Q

5 Major Atomic Theories: Parts of the Quatum/Wave-Mechanical Model

Distance from centre of wave to the bottom of the trough

A

Amplitude

69
Q

5 Major Atomic Theories: Parts of the Quatum/Wave-Mechanical Model

Time for one full wavelength to pass a given point

A

Wave period

70
Q

→ Smallest particle of a chemical element that retain its chemical properties

→ Diameter of this is in the order of 10-8 cm

→ Has a nucles roughly 10-13 cm in diameter and its charge is unique in its character in an elementt

→ Charge is positive

A

Atoms

71
Q

Particles within the Nucleus

Positively charged subatomic particle forming part of the nucleus of an atom and determines **Atomic Number **of an element

A

Proton

72
Q

Particles within the Nucleus

Subatomic particle found in the nucleus of atoms that differs from other subatomic particles, since this has no charge/neutral charge

A

Neutron

73
Q

Particles within the Nucleus

Stable subatomic particle with a negtive electrical charge

A

Electron

74
Q

Modern View of Atom/ forms??

→ Are elements which exist in 2 or more different forms in the same physical state

→ Differ in physical and chemical properties

A

Allotrope

75
Q

Modern View of Atom/ forms??

→ Are atoms of the same element thay have same number of protons but different number of neutrons

A

Isotope

76
Q

Modern View of Atom/ forms??

→ Are atomic species having same mass number but* different atomic number*

→ Differ in chemical properties, same physical properties related to mass

A

Isobars

77
Q

Symbols of the Atom

→ Is the number of protons in the nucleus

→ Located on the lower left side

A

Atomic number

78
Q

Symbols of the Atom

→ Is the sum of the number of protons and neutrons in the nucleus of an atom

→ Located on the upper right side

A

Mass number

79
Q

Is an atom or molecule that carries an electrical charge

A

Ion

80
Q

What are the 2 types of ion?

A
  1. Anion
  2. Cation
81
Q

2 types of ion

Is an atom or a molecule which is negatively charged

Has more number of electrons than protons

A

Anion

82
Q
A
83
Q

→ Is the subdiscipline of chemistry that is concerned with changes in the nucleus of elements.

→ These changes are the source of radioactivity and nuclear power

A

Nuclear Chemistry

84
Q

→Are used to discuss nuclear reactions in depth and we must comprehend how to write balanced equations

→ Sum of the mass # (A) and atomic # (Z) must be the same on both sides

A

Nuclear Equation

85
Q

Various species of atoms whose nuclei contain particular number of protons and neutrons

A

Nuclide

86
Q

Familiarize the rules in Nuclear Stability

A
  1. Nuclides containing odd numbers of both protons and neutrons are least stable (more radioactive)
  2. Nuclides containing even numbers of both protons and neutrons are most stable (less radioactive)
  3. Nuclides containing odd number of protons and even numbers of neutrons (less stable than both even numbers of p and n)
87
Q

Rules in Nuclear Stability

T or F

Nuclides containing odd numbers of both protons and neutrons are least stable (more radioactive)

A

True

88
Q

Rules in Nuclear Stability

T or F

Nuclides containing even numbers of both protons and neutrons are most stable

A

True

89
Q

2 types of ion

Is an atom or a molecule which is positively charged

Has more number of protons than electrons

A

Cation

90
Q

Rules in Nuclear Stability

T or F

Nuclides containing odd number of protons and even number of neutrons are more stable than nuclides with both even number of p and n

A

False (less table since presence of odd number weakens the stability)

91
Q

What are the 3 types of Radioactive Decay?

A
  1. Alpha decay
  2. Beta decay
  3. Gamma de cay
92
Q

3 types of Radioactive Decay

→ Nucleus emits an alha particle wherein alpha particle is essentially a helium nucleus (group of 2 protons and neutrons)

→Very stable

A

Alpha decay

93
Q

3 types of Radioactive Decay

→ Often an electron, but can also be a positron (positively charged particle that is the antimatter equivalent of the electron)

→If an electron is involved, number of neutrons in nucleus decreases by one and number of protons increases by one

A

Beta decay

94
Q

3 types of Radioactive Decay

T or F

In beta decay, If an electron is involved, number of protons in nucleus decreases by one and number of neutrons increases by one

A

False (reverse; If an electron is involved, number of neutrons in nucleus decreases by one and number of protons increases by one)

95
Q

3 types of Radioactive Decay

→The nucleus changes from higher-energy state to a lower level

→When electron changes levels, energy involved is usually a few eV, so a visible or ultraviolet photon is emitted

→ In the nucleus, energy differences between levels are much larger typically a few hundred keV, photon

A

Gamma decay

96
Q

3 concepts under Gamma decay

A process in which a nucleus of an atom splits into 2 or more smaller nuclei as fission products, and usually some by-product particles particles

A

Nuclear Fission

97
Q

3 concepts under Gamma decay

Is the process by which multiple nuclei join together to form a heavier nucleus

A

Nuclear Fusion

98
Q

3 concepts under Gamma decay

is the amount of time needed for a reactant concentration to decrease by half compared to its initial concentration

A

Half-life

99
Q

set of values that describes the state of an electron including its distance from the nucleus, the orientation and type of orbital where it is likely to be found, and its spin

A

Quantum number

100
Q

Are quantum states of the individual electrons in the electron cloud around the single atom

A

Orbital

101
Q

What are the 4 types of quantum numbers?

A
  1. Principal quantum number
  2. Angular quantum numer
  3. Magnetic quantum number
  4. Electron Spin quantum number
102
Q

4 types of quantum numbers

→Values: positive, nonzero integral values (1, 2, 3…)

→ Main energy level or principal shell

→ As this increases:
1. orbital becomes larger
2. (e) becomes farther from nucleus; higher (e) means less tightly bound to the nucleus

A

Principal quantum number (n)

103
Q

4 types of quantum numbers

→Values: 0, n-1 (for each value of N)
→ Sublevel/Subshell
→ Related to the shape of the orbital

A

Angular quantum number (I)

104
Q

4 types of quantum numbers: Angular quantum number

0:
1:
2:
3:

Identify appropriate letter designation for given angular quantum number

A

0: s
1: p
2: d
3: f

105
Q

4 types of quantum numbers

→ Values: I to -l including zero
→ Related to the orientation in space of the angular momentum associated with the orbital

A

Magnetic quantum number (m1)

106
Q

4 types of quantum numbers: Magnetic quantum number

Defined as orbitals having the same energies (ex. three p-orbitals having the same energy)

A

Degenerate orbitals

107
Q

4 types of quantum numbers

→ Values: +1/2, -1/2
→ Describes spin for a given electron
→ The value does not depend on any of the three quantum numbers

A

Electron Spin quantum number (ms)

108
Q

4 types of quantum numbers: Application

Identify principal quantum number (n), angular momentum (I), magnetic quantum number (m1), and spin quantum number (ms):
1s^2 2s^2 2p^5

A

n = 2
l = 1 (remember: s-0, p-1, d-2, f-3)
m1 = 0
ms = -1/2

109
Q

4 types of quantum numbers: Magnetic quantum number

Identify associated magnetic quantum number (m1) for the orbital notation:

1s, 2s, 3s, 4s:

2p, 3p, 4p:

3d, 4d:

4f:

A

1s, 2s, 3s, 4s: 0

2p, 3p, 4p: -1, 0, +1

3d, 4d: -2, -1, 0, +1, +2

4f: -3, -2, -1, 0, +1, +2, +3

s - 0
p - 1
d - 2
f - 3

110
Q

The order in which electrons are placed into the orbitals is based on the order of their energy

A

Aufbau principle

111
Q

T or F

Aufbau principle states that lowest energy orbitals fill first

A

T

112
Q

If you read this card

A

Familiarize/Draw the electronic configuration acc. to aufbau principle NOW NA

113
Q

→ Arranged in order of atomic number

→ Contains a period and a group

A

Periodic Table

114
Q

Periodic Table

A horizontal row in the periodic table

A

Period

115
Q

Periodic Table

Is a vertical row of the periodic table

A

Group

116
Q

Familiarize the groups in the periodic table

A

Group 1: Alkali metals
Group 2: Alkaline earth metals
Group 17: Halogens
Group 18: Noble gases

117
Q

Periodic Table

These properties** decrease** from left to right, and **increase ** from top to bottom

A

Atomic size, Tendency to form Cation, Metallic Character

118
Q

Periodic Table

These properties increase from left to right, and decrease from top to bottom

A

Ionization energy, Affinity for electrons, Tendency to form Anion, Electronegativity

**note: **anything pertaining to electrons increases from left to right but decreases from top to bottom

119
Q

Atomic Size

Radius of an atom when covalently bonded to other atoms

A

Covalent radius

120
Q

Atomic Size

One-half of the distance between the nuclei of two atoms in crystal or bvetween two adjacent ions in the metallic lattice

A

Metallic Radius

121
Q

Atomic Size

Energy needed to remove an electron from an aton or molecule to infinity

A

Ionization energy

122
Q

Atomic Size

The energy given off when a neutral atom in the gas phase gains an extra electron to form a negatively charged ion

A

Electron affinity

123
Q

Atomic Size

→ Chemical property that descirbes the tendency of an atom or a functional group to attract electron towards itself.

→ Increases from left to right, decreases from top to bottom

A

Electronegativity

124
Q

Chemical Language and Shorthand

→ Consists of two different elements

→ Has two types: Molecular, Ionic

A

Binary Covalent Compounds

125
Q

Chemical Language and Shorthand: Binary Covalent Compounds

Type binary compound wherein it consists of two nonmetals

A

Molecular binary compounds

126
Q

Chemical Language and Shorthand: Binary Covalent Compounds

Type binary compound wherein it consists of a metal and nonmetal

A

Ionic binary compound

127
Q

Familiarize the non metals in the periodic table

A

Hydrogen, Helium, Carbon, Nitrogen, Oxygen, Fluorine, Neon, Phosphorus, Sulfur, Chlorine, Argon, Selenium, Bromium, Krypton, Iodine, Xenon, Radon, Oganesson

remember these non metals to determine if binary or ionic

Binary = 2 nonmetals
Ionic = nonmetal + metal

– highlighted portion are most common –

128
Q

Familiarize the transition metals

remember that in naming transition metals there are roman numerals

A

Scandium, Titanium, Vanadium, Chromium, Manganese, Iron, Cobalt, Nickel, Copper, Zinc, Yttrium, Zicronium, Niobium, Molybedinium, Technetium, Rhodium, Palladium, Silver, Cadmium, Hafnium, Tantallum, Tungsten, Rhenium, Osmium, Iridium, Platinum, Gold, Mercury, RF to CN (pakicheck nalang periodic table tinamad na ako)

remember that in naming transition metals there are roman numerals

– highlighted portion are most common –

129
Q

Familiarize Group 1A (alkali metals) and their charge

for naming compounds

A

Hydrogen, Lithium, Sodium, Potassium, Rubidium, Caesium

Charge: +1

130
Q

Familiarize the Group 2A (alkaline earth metals) and their charge

for naming compounds

A

Berillium, Magnesium, Calcium, Strontium, Barium

Charge: +2

131
Q

Familiarize the Group 3A and their charge

for naming compounds

A

Aluminum, Gallium

Charge: +3

132
Q

Familiarize the Group 4A and their charges

for naming compounds

A

Tin: +2, +4
Lead, +3, +4

133
Q

Familiarize the Group 7A (halogens)

for naming compounds

A

Fluorine, Chlorine, Bromium, Iodine

Charge: -1

134
Q

Familiarize the Group 6A and their charge

for naming compounds

A

Oxygen, Sulfur, Sellenium

Charge: -2

135
Q

Familiarize the Group 5A and their charges

for naming compounds

A

Nitrogen, Phosphorus

Charge: -3

136
Q

Naming Binary Acids

What prefix should the binary acid have?

A

“hydro”

137
Q

Naming Binary Acids

What sufix should the binary acid have?

A

“-ic acid”

138
Q

OH-

for naming compounds

A

Hydroxide

139
Q

O2^-2

for naming compounds

A

Peroxide

141
Q

SO4^-2

for naming compounds

A

Sulfate

142
Q

SO3^-2

for naming compounds

A

Sulfite

143
Q

HSO4^-

for naming compounds

A

Hydrogen sulfate

144
Q

HSO3^-

for naming compounds

A

Hydrogen sulfite

145
Q

PO4^-3

for naming compounds

A

Phosphate

146
Q

PO4^-2

for naming compounds

A

Hydrogen phosphate

147
Q

NO3^-

for naming compounds

A

Nitrate

148
Q

NO2^-

for naming compounds

A

Nitrite

149
Q

CH3COO^-

for naming compounds

A

Acetate

150
Q

CrO4^-2

for naming compounds

A

Chromate

151
Q

ClO4^-

for naming compounds

A

Perchlorate

152
Q

ClO3^-

for naming compounds

A

Chlorate

153
Q

ClO2^-

for naming compounds

A

Chlorite

154
Q

ClO^-

for naming compounds

A

Hypochlorite

155
Q

BrO4^-

for naming compounds

A

Perbromate

DOST Review (8 decks)

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