CHEMISTRY Flashcards
(154 cards)
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
2
Q
Branches of Chemistry (5)
Deals with the separation, identification and quantification of chemical substances (analytes) in a gicven sample
A
Analytical chemistry
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
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
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
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
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
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
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
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
11
Q
This refers to the closeness of a measured value to a standard or known value
A
Accuracy
12
Q
This refers to closeness of two or more measurements to each other aka repeatability
A
Precision
13
Q
Is anything that occupies physical space and has mass and inertia
A
Matter
14
Q
What are the 2 kinds of Matter?
A
Pure substance and Mixture
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
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
17
Q
2 kinds of matter:
2 Types of Pure Substances
A
Elements and Compounds
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
19
Q
2 Types of Pure Substances: Compound
3 types of compounds
A
- Ionic compounds
- Covalent Compounds
- Covalent Network Substances
20
Q
3 types of compounds
Are compounds composed of disscrete ions or charged species
A
Ionic compounds
21
Q
3 types of compounds: Ionic Compound
Familiarize the properties of ionic compounds
2 Types of Pure Substances
A
- Solid
- High melting and boiling points
- Soluble in polar liquids like water (not in nonpolar)
- Hard
- Very reactive
22
Q
3 types of compounds
Molecule formed by covalent bonds
A
Covalent compound
23
Q
Bonds
Type of bond which atoms share one or more pairs of valence electrons
A
Covalent bond
24
Q
3 types of compounds
Familiarize the properties of Covalent Compound
A
- High volatility
- Weak bonds
- Insoluble in water/polar liequids
- Low melting point
- Form a molecule
- Form between two nonmetals
25
# 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
Covalent Network Substances
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# 3 types of compounds: Covalent Network Substances
Familiarize the properties of Covalent Network Substances
1. High melting point
2. Very hard
3. Non conducting
4. Insoluble in any solvent
28
What are the 2 major properties of matter?
1. Physical properties
2. Chemical properties
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What are the 2 properties under physical properties?
1. Intensive property
2. Extensive property
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# 2 major properties of matter
Can be observed or measured without changing the composition of matter
Physical Property
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# 2 major properties of matter
Decribe the characteristic ability of a substance to react to form new substances
| Flammability, Susceptibility to corrosion
Chemical Property
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# 2 properties under Physical Property
A physical property that will be the same regardless of the amount of matter
Intensive Property (density, color, luster, odor, malleability, conductivity, hardness, ductility, boiling point, melting point)
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# 2 properties under Physical Property
A physical property that will change if the amount of matter changes
Extensive property
| MASS, VOLUME, WEIGHT (M V W)
## Footnote
MEMORIZEEEE
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2 kinds of changes in matter
1. Physical Change
2. Chemical Change
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# 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
Physical change
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# 2 kinds of changes in matter: Physical Change
Types of Physical Changes
1. Sublimation
2. Melting
3. Freezing
4. Boiling/Evaporation
5. Condensation
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# 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
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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# 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
Chemical Change
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# 2 kinds of changes in matter: Chemical change
Types of Chemical Changes
1. Combination/synthesis
2. Decomposition
3. Substitution/siNGLE Replacement
4. Double Discplacement
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# Types of Chemical Changes
Two or more reactants **unite** to form a single product
Combination or Synthesis
| 2Na(s) + Cl2(g) → 2NaCl(s)
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# Types of Chemical Changes
A single reactant is **broken down** into two or more products
| opposite reaction of combination
Decomposition
| 2HgO(s) → 2Hg(l) + O2(g)
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# Types of Chemical Changes
A **single** free element replaces or is** substituted** for one of the elements in a compound
Substitution or Single Replacement
| Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g)
## Footnote
Cl2 is substituted / the free element
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# 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
Double displacement reaction
| AgNO3 + NaCl → AgCl + NaNO
## Footnote
Exchange of partners yuck
46
What are the 2 types of mixtures
1. Homogenous
2. HETERogeneous
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# 2 types of mixtures
Two or more substances that form the mixture are evely distributed througout the mixture
| Ex. Vinegar (ethanoic acid + water)
Homogenous mixture
| bading
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# 2 types of mixtures
Two or more substances that form the mixture are not evenly distributed throughout the mixture
| Ex. water and oil
## Footnote
TUBIG AT LANGISSSSSSSS~~~ iykyk
Heterogenous mixtures
| straight ka aw
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# Mixture:
Familiarize the Solubility rules
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)
50
What are the following 3 Laws of Chemical Combination
1. Law of Conservation of Mass
2. Law of Definite Proportion or Composition
3. Law of Multiple Proportion
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# 3 Laws of Chemical Combination
States that matter cannot be created or destroyed in a chemical reaction
Law of Conservation of Mass
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# 3 Laws of Chemical Combination
States that chemical compounds are formed of constant and defined ratios of elements as determined by mass
Law of Definite Proportion or Composition
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# 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
Law of Multiple Proportion
56
What are the 5 Major Atomic Theories?
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
57
# 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
John Dalton's Atomic Theory
**REMINDER:** JD's theory focused on the definition/properties of an atom, element, compound
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# 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
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
59
# 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)
Rutherford's Nuclear Atom Model (Alpha scattering Experiment)
**REMINDER:** Mainly stated the existence of (+) charged nucleus and orbit of (-) charged
60
# 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**
Rutherford's Nuclear Atom Model (Alpha scattering Experiment)
**REMINDER:** Mainly stated the existence of (+) charged **nucleus** and **orbit **of (-) charged
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# 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
Bohr's Solar System Model of the Atom
**REMINDER:** Stated the positioning of electrons, energy of orbit, Light/Energy is emitted or absorbed
62
# 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
Quantum or Wave-Mechanical Model
**REMINDER:** Stated that elrctrons are in 3d region/wave??
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# 5 Major Atomic Theories: Parts of the Quatum/Wave-Mechanical Model
Highest point of the wave
Crest
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# 5 Major Atomic Theories: Parts of the Quatum/Wave-Mechanical Model
Lowest point of the wave
Trough
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# 5 Major Atomic Theories: Parts of the Quatum/Wave-Mechanical Model
Distance from one crest and trough to the next
Wavelength
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# 5 Major Atomic Theories: Parts of the Quatum/Wave-Mechanical Model
Height from trough to crest
Wave Height
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# 5 Major Atomic Theories: Parts of the Quatum/Wave-Mechanical Model
Ratio of wave height to wavelength
Wave steepness
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# 5 Major Atomic Theories: Parts of the Quatum/Wave-Mechanical Model
Distance from centre of wave to the bottom of the trough
Amplitude
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# 5 Major Atomic Theories: Parts of the Quatum/Wave-Mechanical Model
Time for one full wavelength to pass a given point
Wave period
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→ 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
Atoms
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# Particles within the Nucleus
Positively charged subatomic particle forming part of the nucleus of an atom and determines **Atomic Number **of an element
Proton
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# 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
Neutron
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# Particles within the Nucleus
Stable subatomic particle with a negtive electrical charge
Electron
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# 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
Allotrope
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# Modern View of Atom/ forms??
→ Are atoms of the same element thay have *same number of protons* but *different number of neutrons*
Isotope
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# 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
Isobars
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# Symbols of the Atom
→ Is the number of protons in the nucleus
→ Located on the lower left side
Atomic number
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# 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
Mass number
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Is an atom or molecule that carries an electrical charge
Ion
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What are the 2 types of ion?
1. Anion
2. Cation
81
# 2 types of ion
Is an atom or a molecule which is negatively charged
Has more number of electrons than protons
Anion
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→ 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
Nuclear Chemistry
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→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
Nuclear Equation
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Various species of atoms whose nuclei contain **particular number** of protons and neutrons
Nuclide
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Familiarize the rules in Nuclear Stability
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
# Rules in Nuclear Stability
T or F
Nuclides containing odd numbers of both protons and neutrons are least stable (more radioactive)
True
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# Rules in Nuclear Stability
T or F
Nuclides containing even numbers of both protons and neutrons are most stable
True
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# 2 types of ion
Is an atom or a molecule which is positively charged
Has more number of protons than electrons
Cation
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# 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
False (less table since presence of odd number weakens the stability)
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What are the 3 types of Radioactive Decay?
1. Alpha decay
2. Beta decay
3. Gamma de cay
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# 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
Alpha decay
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# 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
Beta decay
94
# 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
False (reverse; If an electron is involved, number of **neutrons in nucleus decreases** by one and **number of protons increases** by one)
95
# 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
Gamma decay
96
# 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
Nuclear Fission
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# 3 concepts under Gamma decay
Is the process by which multiple nuclei join together to form a heavier nucleus
Nuclear Fusion
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# 3 concepts under Gamma decay
is the amount of time needed for a reactant concentration to decrease by half compared to its initial concentration
Half-life
99
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
Quantum number
100
Are quantum states of the individual electrons in the electron cloud around the single atom
Orbital
101
What are the 4 types of quantum numbers?
1. Principal quantum number
2. Angular quantum numer
3. Magnetic quantum number
4. Electron Spin quantum number
102
# 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
Principal quantum number (n)
103
# 4 types of quantum numbers
→Values: 0, n-1 (for each value of N)
→ Sublevel/Subshell
→ Related to the shape of the orbital
Angular quantum number (I)
104
# 4 types of quantum numbers: Angular quantum number
0:
1:
2:
3:
| Identify appropriate letter designation for given angular quantum number
0: s
1: p
2: d
3: f
105
# 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
Magnetic quantum number (m1)
106
# 4 types of quantum numbers: Magnetic quantum number
Defined as orbitals having the same energies (ex. three p-orbitals having the same energy)
Degenerate orbitals
107
# 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
Electron Spin quantum number (ms)
108
# 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
n = 2
l = 1 (remember: s-0, p-1, d-2, f-3)
m1 = 0
ms = -1/2
109
# 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:
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
The order in which electrons are placed into the orbitals is based on the order of their energy
Aufbau principle
111
T or F
Aufbau principle states that lowest energy orbitals fill first
T
112
If you read this card
Familiarize/Draw the electronic configuration acc. to aufbau principle NOW NA
113
→ Arranged in order of atomic number
→ Contains a period and a group
Periodic Table
114
# Periodic Table
A horizontal row in the periodic table
Period
115
# Periodic Table
Is a vertical row of the periodic table
Group
116
Familiarize the groups in the periodic table
Group 1: Alkali metals
Group 2: Alkaline earth metals
Group 17: Halogens
Group 18: Noble gases
117
# Periodic Table
These properties** decrease** from left to right, and **increase ** from top to bottom
Atomic size, Tendency to form Cation, Metallic Character
118
# Periodic Table
These properties increase from left to right, and decrease from top to bottom
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
# Atomic Size
Radius of an atom when covalently bonded to other atoms
Covalent radius
120
# Atomic Size
One-half of the distance between the nuclei of two atoms in crystal or bvetween two adjacent ions in the metallic lattice
Metallic Radius
121
# Atomic Size
Energy needed to remove an electron from an aton or molecule to infinity
Ionization energy
122
# Atomic Size
The energy given off when a neutral atom in the gas phase gains an extra electron to form a negatively charged ion
Electron affinity
123
# 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
Electronegativity
124
# Chemical Language and Shorthand
→ Consists of two different elements
→ Has two types: Molecular, Ionic
Binary Covalent Compounds
125
# Chemical Language and Shorthand: Binary Covalent Compounds
Type binary compound wherein it consists of two nonmetals
Molecular binary compounds
126
# Chemical Language and Shorthand: Binary Covalent Compounds
Type binary compound wherein it consists of a metal and nonmetal
Ionic binary compound
127
Familiarize the non metals in the periodic table
**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
## Footnote
Binary = 2 nonmetals
Ionic = nonmetal + metal
-- highlighted portion are most common --
128
Familiarize the transition metals
| remember that in naming transition metals there are roman numerals
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
## Footnote
-- highlighted portion are most common --
129
Familiarize Group 1A (alkali metals) and their charge
| for naming compounds
Hydrogen, Lithium, Sodium, Potassium, Rubidium, Caesium
Charge: +1
130
Familiarize the Group 2A (alkaline earth metals) and their charge
| for naming compounds
Berillium, Magnesium, Calcium, Strontium, Barium
Charge: +2
131
Familiarize the Group 3A and their charge
| for naming compounds
Aluminum, Gallium
Charge: +3
132
Familiarize the Group 4A and their charges
| for naming compounds
Tin: +2, +4
Lead, +3, +4
133
Familiarize the Group 7A (halogens)
| for naming compounds
Fluorine, Chlorine, Bromium, Iodine
Charge: -1
134
Familiarize the Group 6A and their charge
| for naming compounds
Oxygen, Sulfur, Sellenium
Charge: -2
135
Familiarize the Group 5A and their charges
| for naming compounds
Nitrogen, Phosphorus
Charge: -3
136
# Naming Binary Acids
What prefix should the binary acid have?
"hydro"
137
# Naming Binary Acids
What sufix should the binary acid have?
"-ic acid"
138
OH-
| for naming compounds
Hydroxide
139
O2^-2
| for naming compounds
Peroxide
141
SO4^-2
| for naming compounds
Sulfate
142
SO3^-2
| for naming compounds
Sulfite
143
HSO4^-
| for naming compounds
Hydrogen sulfate
144
HSO3^-
| for naming compounds
Hydrogen sulfite
145
PO4^-3
| for naming compounds
Phosphate
146
PO4^-2
| for naming compounds
Hydrogen phosphate
147
NO3^-
| for naming compounds
Nitrate
148
NO2^-
| for naming compounds
Nitrite
149
CH3COO^-
| for naming compounds
Acetate
150
CrO4^-2
| for naming compounds
Chromate
151
ClO4^-
| for naming compounds
Perchlorate
152
ClO3^-
| for naming compounds
Chlorate
153
ClO2^-
| for naming compounds
Chlorite
154
ClO^-
| for naming compounds
Hypochlorite
155
BrO4^-
| for naming compounds
Perbromate
