Chemistry Winter Quizlet
-20⁰C = ____⁰F (Round to the nearest degree)
-4⁰F
57 mL = ______ L
0.057
How many significant digits area in the number 0.009?
1
Multiply the following three numbers and report your answer to the correct number of significant figures: 0.020 cm x 50 cm x 11.1 cm
1 x 10 cm³
Specific Heat
1. A physical property of a substance 2. The heat capacetiy of 1 gram of a substance.
1cm³ = ___ mL
1cm³ = 1mL
Centi
1m=10²cm. Unit prefix meaning one hundredth. Symbol = c
Milli
1m=10³mm. Unit prefix meaning one thousandth. Symbol = m
Micro
1m=10⁶µm. Unit prefix meaning one millionth. Symbol = µ
Nano
1m=10⁹nm. Unit prefix meaning one billionth. Symbol = n
2 cm = ______mm
20
Compound
A chemical compound is a pure chemical substance consisting of two or more different chemical elements that can be separated into simpler substances by chemical reactions.
exothermic reaction
A chemical reaction that releases energy to its surroundings
Tyndall
A colloid is one of the three primary types of mixtures, with the other two being a solution and suspension. Scatters light, does not settle on standing. A subtype of heterogeneous mixture.
Suspension
A colloid is one of the three primary types of mixtures, with the other two being a solution and suspension. Separates on standing. A subtype of heterogeneous mixture.
chemical formula
A combination of chemical symbols and numbers to represent a substance
Mole
A counting unit used to calculate objects that are very small in size and large in number
Temperature
A measurement of the average kinetic energy of a molcule
Metric System
A measurement system based on the number 10 which uses prefix to make the unit larger or smaller than the base.
Molecule
A molecule is two or more atoms join together chemically.
Significant figures
All certain digit and one estimated digit.
Wood Burning
Chemical Change
f block
Covers the Lathanides and Actinides
d block
Covers the Transition Metals
s block
Covers the alkaline metals and alkaline earth metals. It is spherically symmetrical
dichromate ion
Cr2O7 2-
chromate ion
CrO4 2-
Allotrope
Different forms of the same element. Pure substances!
Atomic Radii
Distance from nucleus to outermost e⁻shell. - ↑ down a group b/c more e⁻ are added to shell, ↓ across a period b/c more e⁻ and p⁺ are added & effective nuclear charge (e.n.c) is greater.
Techniques for Separating Mixtures
Distillation - separate two liquids w/ different boiling points Filtration - porous barrier to separate solids from liquids
Converting from atoms to moles
Divide the number of particles by Avogadro's number to determine the number of moles
hydrogen carbonate ion
HCO3 -
hydrogen phosphate ion
HPO4 2-
hydrogen sulfate ion
HSO4 -
Desired bunsen burner flame
Is blue with and inner and outer cone
ammonium ion
NH4 +
Hund's Rule
The Half Rule; No orbitals shall have a two electrons occupying it until all the orbitals in a subshell have been filled.
Tyndall Effect
The Tyndall Effect is the effect of light scattering in many directions in colloidal dispersion, while showing no light in a true solution.
Energy
The ability to do work
Heat Capacity
The amount of heat needed to raise the temperature of the object by 1 degree Celsius.
Mass
The amount of matter in an object. SI unit = kg
Volume
The amount of space that a substance or object occupies. SI = m³
True or false? All compounds are molecules but not all molecules are compounds.
True!
Compounds
Two or more elements combined CHEMICALLY; pure substance that CAN be separated by chemical means; can be identified by a chemical formula that is always the same
Mixtures (of Matter)
Types of Mixtures (Homogeneous & Heterogeneous)
Homogeneous Mixture
Uniform,constant composition; components are in a single phase; A.K.A: solutions
Z (number of protons)
atomic number
Dalton's Atomic Theory
1. All matter (materials) consists of very small particles called atoms. 2. An element consists of atoms of one type only 3. Compounds consist of atoms of more than one element and are formed by combining atoms in whole-number ratios. 4. In a chemical reaction, atoms are neither created nor destroyed
Heat of Fusion
1. The amount of heat needed to convert a solid at its melting point to a liquid. 2. The amount of heat needed to convert a unit mass of a substance from solid to liquid at its melting point 3. q= mHfus 4. M=Mass 5. Hfus= Heat of Fusion Heat of Fusion: 334 J/g 6. q= Heat in Joules
Heat of Vaporization
1. The amount of heat needed to convert a unit mass of a substance from its liquid phase to its vapor phase at a constant temperature. 2. q= mHvap 3. q= Heat(in Joules) 4. m= mass 5. Hvap= Heat of Vaporization 2260 J/g
Heat
1. The measure of the amount of energy transferred from one substance to another. 2. Heat is measured in Calories or Joules.
What are the 3 States of Matter?
1. solid 2. liquid 3. gas
water's density?
1.00g/mL
Kilo
10³m=1 km. Unit prefix meaning one thousand. Symbol = k
Mega
10⁶m=1 Mm. Unit prefix meaning one million. Symbol = M
Giga
10⁹m= 1Gm. Unit prefix meaning one billion. Symbol = G
64⁰F = ____⁰C (Round to the nearest degree)
18⁰C
Equivalence statement
2 statements with different units that are equal. Ex: 1 inch = 2.54 cm
3.5 g = ______mg
3,500
The speed of light in a vacuum is exactly 299,792,458 meters per second. Write this number in scientific notation with the coefficient rounded to the hundredths place.
3.00 × 10⁸
Write 3,465 in scientific notation.
3.465×10³
How many significant digits are in the number 0.000005721?
4
Water (H₂0) Specific Heat
4.18 J/g °C or 1.00 cal/g °C
Write 45,870,320 in scientific notation.
4.587032 × 10⁷
Find the sum of 23.6 liters, 4.75 liters, 12.065 liters, and 9.11 liters using the correct precision.
49.5 L
Divide the following numbers and report your answer to the correct number of significant figures: 0.530 g / 0.1010 mL = ?
5.25 g/mL
67.2 m = ______ cm
6,720
7,939 mg = ______ g
7.939
Which symbol makes the following statement true? 7,500 ______ 7.5 × 10³
=
Which symbol makes the following statement true? 568 ______ 5.1 × 10²
>
coefficient
A number placed in front of a formula in an equation to indicate the number of molecules of a substance
subscript
A number written slightly below and to the right of a chemical symbol that shows how many atoms of an element are in a compound.
Units
A particular amount (g, L, km)
Dimensional Analysis
A problem solving method scientists use to convert units of measurement. Uses equivalence statements as ratios and cross out units.
chemical reaction
A process that produces one or more substances that are different from the original substance (like baking or burning)
Chemical property
A property or characteristic of a substance that is observed during a reaction in which the chemical composition or identity of the substance is changed:
Pure substance
A pure element or compound contains only ONE substance, with no other substances mixed in. Impure materials are mixtures of elements, mixtures of compounds, or mixtures of elements and compounds.
endothermic reaction
A reaction that absorbs energy in the form of heat.
chemical equation
A representation of a chemical reaction that uses symbols to show the relationship between the reactants and the products
Quantum Numbers
A series of numbers to classify location of electron
Precipitate
A solid that forms from a solution during a chemical reaction.
products
A substance formed as a result of a chemical reaction
reactants
A substance or molecule that participates in a chemical reaction
Electron Affinity (EA)
Ability to acquire e. When atom accepts electron, energy is released (meaning it's negative) - ↑ up a group b/c atomic size decreases upwards, ↑ across a group b/c of increased enc.
Electronegativity
Ability to attract shared e⁻ to itself. - ↓ down a group b/c greater the size of atom, more electron shielding occurs, ↑ across a period. Group 18 does not apply.
silver ion
Ag +
Alloy
An alloy is a solid mixture that contains two or more metals (occasionally a non-metal like carbon) mixed together.
Atom
An atom is the smallest constituent unit of matter that has the properties of a chemical element.
Element
An element is a type of atom that is defined by its atomic number (#of protons in its nucleus). Ex: Au, S, Fe
Conversion Factor
An equivalence statement written as a ratio: 1inch/2.54cm or 2.54cm/inch
Mass Spectrometer
An instrument used to determine the relative atomic mass of an element.
Calorimeter
An object used to measure the heat in a chemical reaction.
Chemical Change
Any change that results in the formation of new chemical substances. At the molecular level, chemical change involves making or breaking of bonds between atoms.
Matter
Anything that has mass and occupies space.
Isotopes
Atoms of same elements with different numbers of neutrons.
barium ion
Ba 2+
Physical change verbs
Bend, tear, boil, freeze, melt
bromide ion
Br -
Chemical change verbs
Burn, tarnish, combust, cook, digest
acetate ion
C2H3O2 -
oxalate ion
C2O4 2-
cyanide ion
CN -
carbonate ion
CO3 2-
calcium ion
Ca 2+
Physical change
Changes that result in a difference in display without changing the composition.
Proton
Charge: +1 Mass: 1.660539 x 10^-24g
Electron
Charge: -1 Mass: 9.10938291 × 10-28 grams
Neutron
Charge: 0 Mass: 1.660539 x 10^-24g Discovered by British physicist James Chadwick in 1932. Found Beryllium to emit neutrons and based on mass calculations, he was able to prove that the particles were in fact neutrons and not gamma rays as previously though.
Adding Aluminum foil to copper chloride solution
Chemical Change
Burning magnesium metal
Chemical Change
Dynamite exploding
Chemical Change
Giving your hair a permanent
Chemical Change
Iron Rusting
Chemical Change
Milk souring
Chemical Change
Passing an electric current through water
Chemical Change
Silver tarnishing
Chemical Change
Corrosive Liquid
Chemical Property
Gasoline is flammable
Chemical Property
Helium will not form compounds
Chemical Property
Inert gas
Chemical Property
Sodium has the ability to combine with chlorine
Chemical Property
chloride ion
Cl -
Heterogeneous Mixtures
Composition is NOT uniform; individual substances are distinct; components are not blended smoothly
p block
Covers column of Boron to the Noble gases. It is dumbbell shaped.
Density
D=M/V. The ratio between mass and volume.
____________ is a technique used to separate elements in a compound. This process breaks chemical bonds.
Electrolysis
Pure Substances can be either __________ or __________
Elements / Compounds
Continuous Spectrum
Emitting a range of wavelengths continuously. Such as a rainbow created when light penetrates a glass prism.
Law of Conservation of Energy
Energy cannot be created or destroyed.
Potential energy
Energy due to position.
Exothermic
Energy moves from system to the surroundings.
Endothermic
Energy moves from the surroundings to the system.
Ionization Energy (IE)
Energy required to remove an e⁻from gas phase. "Jumps" really high once a stable ion is formed. - ↑ up a group b/c atom size decreases and becomes hard to pull e⁻ away , ↑ across a group b/c greater enc means stronger pull to nucleus.
Physical property
Ex: luster, odor, color, density, temperature, boiling point, malleability, ductility
fluoride ion
F -
Filtration
Filtration is a separation technique that is used to separate heterogeneous mixtures solid that has not dissolved in a liquid (for example a precipitate).
Fills the entire volume of a container
Gas
Converting grams to moles
Given 237g of H2O, how many moles?
Molar Mass of a single molecule
Grams per mole
Alkali Metals
Group 1 elements: Most chemically reactive, very soft, forms ions with Group 17 elements, and rapidly oxidize.
Alkaline Earth Metals
Group 2 elements: Forms basic solutions w/ water, hard, have higher mp, bp, and density than Group 1.
Halogens
Group 7 elements: salt formers. all diatomic molecules, except At; all nonmetals, form ionic salts with Group 1 elements
Noble Gases
Group 8 elements: least reactive (inert) of all elements; all nonmetals, have a full outer shell.
hydride ion
H -
dihydrogen phosphate ion
H2PO4 -
Metalloids
Have intermediate properties of metals and nonmetals.
Quantum Mechanical Model of the Atom
Heisenberg, de Broglie, and Schrodinger created this. The truth is, electrons have wave-length properties and occupy orbitals (each holds only 2 electrons).
mercury (II) ion
Hg 2+
mercury (I) ion
Hg2 2+
Solution
Homogeneous mixture.
iodide ion
I -
Law of Multiple Proportion
If two elements X and Y combine in different ways to form more than one compound, the masses of X that combine with a fixed mass of Y can be expressed as a ratio of small whole numbers (Ex. When Mass of N: 1.00g N₂O -> Mass of O: 0.571g; NO -> Mass of O: 1.14g; NO₂ -> Mass of O: 2.28g; NO₃ -> Mass of O: 4.57g) - John Dalton, 1804
Heisenberg Uncertainty Principle
It states that it is impossible to pinpoint location of electron and the momentum of a particle simultaneously.
Cathode Ray Tube
J.J. Thomson worked on cathode rays which he suggested consists of very small negatively charged particles called electrons. He then developed the Plum Pudding Model.
Heterogeneous Mixtures - examples
Juice with pulp; fruit salad, chef's salad, Greek salad; vegetable soup; oil/vinegar/soil and water; crunchy peanut butter; carbonated soft drinks
Kelvin Scale
K = C + 273.15. A temperature scale with zero degrees K defined as absolute zero (no molecular movement)
Non-metals
Lack all physical properties of metals; brittle
lithium ion
Li +
Has a definite volume but it takes the shape of a container
Liquid
Aufbau Principle
Literally building up from the bottom; e⁻ fills lowest energy level first.
Law of the Conservation of Mass
Mass is neither created nor destroyed. Therefore the total mass of matter following a chemical reaction is equal to the total mass of matter before the start of the reaction. Brought to you by Antoine Lavoisier!
Mass to Particle Conversions
Mass must first be converted to moles and then moles to particles Can be combined into one equation for a mass to particle conversion
Molar Mass of a Compound
Mass of one mole of formula units For example: H2O
law of conservation of mass
Matter is not created or destroyed in any chemical or physical change
rate of reaction
Measure of how fast a chemical reaction occurs
Distilation
Method for separating liquid mixtures into their individual components by boiling.
magnesium ion
Mg 2+
permanganate ion
MnO4 -
Metals
Most elements are this; conducts heat and electricity, is malleable, ductile, and lustrous
Converting from moles to atoms
Multiply the number of moles by Avogadro's number to determine the number of atoms or particles for a particular element
nitrite ion
NO2 -
nitrate ion
NO3 -
sodium ion
Na +
Molar Mass / Molecular Weight
Number of atoms X Grams per mole
Valence Electrons
Number of outermost e⁻; determine chemical properties
oxide ion
O 2-
hydroxide ion
OH -
Effective Nuclear Charge
Overall attraction that e⁻ experiences.
phosphate ion
PO4 3-
Absorption Spectrum
Pattern of dark lines against a coloured background.
To find an element look on the _________ ________
Periodic Table
Density, color, odor, hardness, shape, weight, change of state (melting / freezing / evaporation / condensation / sublimation / deposition / dissolving) are all examples of _____________ properties
Physical
Boiling alcohol
Physical Change
Cutting your hair
Physical Change
Dry ice changing to carbon dioxide gas
Physical Change
Iodine subliming
Physical Change
Sugar dissolving in water
Physical Change
Water evaporating
Physical Change
Water vapor condensing
Physical Change
Wood being carved
Physical Change
Car oil is a viscous liquid
Physical Property
Hard mineral
Physical Property
Malleable Metal
Physical Property
Shiny Metal
Physical Property
red powder
Physical Property
silly putty is an amorphous solid
Physical Property
the freezing point of water is 0˚C
Physical Property
Noble Gas Configuration
Preceding noble gas represents core e⁻ of atom (ex. CA = [Ar]4s²
Paramagnetism
Property of attraction to magnetic field. atoms of these substances have unpaired e⁻
Diamagnetism
Property of repulsion to magnetic field. atoms of these substances have paired e⁻.
Chemical Properties
Reacts or doesn't react Forms a new compound... a new color is produced...a gas is formed...a solid is formed from two liquids
Rounding off
Reducing the digits in a number while trying to keep its value similar.
sulfide ion
S 2-
sulfite ion
SO3 2-
sulfate ion
SO4 2-
Distillation
Separation of two or more substances based on boiling point.
Emission Spectrum
Series of lines against a dark background.
Radioisotopes
Short for radioactive isotopes. Unstable atomic nucleus and emit energy and particles when it changes to a more stable form. Goes through radioactive decay. Examples of human use: Positron Emission Tomography (PET) Cobalt-60 (emits gamma rays to treat cancer) Carbon-14 (Half life: 5730, archaeology)
tin (IV) ion
Sn 4+
Definite shape, definite volume.
Solid
Electromagnetic Spectrum (EMS)
Spectrum of wavelengths that comprise the various types of electromagnetic radiation (ex. radio waves, microwaves, infrared radiation, ultraviolet radiation, X-rays, and gamma rays.)
Pauli Exclusion Theory
States that any orbital can hold a maximum of two electrons of opposite spin.
Modern View of the Atom
Stresses that the nucleus (of protons and neutrons) take up the center and is extremely small. Just as the nucleus accounts for the weight, the electrons around it account for the space.
SI Units
System of units of measurements that is widely used all over the world. There are only four units that we covered in depth: Mass (kg), length (m), volume m³, temperature (k)
Law of Definite Proportion
The law states that a compound always has the same proportions of elements by mass. For example, if you measure the mass of sulphur and oxygen in sulphur tri-oxide, SO₃ will always contain 1 part sulphur and 3 parts oxygen by mass.
Atomic Mass Units
The mass of a single atom of an element 1 a.m.u. = 1.66 X 10^-24 grams
Avogadro's Number
The number of representative particles in one mole of a substance 6.02 X 10^23
Formula Units
The simplest ratio of ions for the compound Used to describe compounds rather than single elements
The hottest part of an optimal flame is:
The top of the inner cone
Conversion Factors
To convert mass to particles follow down arrows To convert particles to mass follow up arrows
Isoelectronic
Used to describe atoms that have same e⁻ configuration (Ne = Na⁺)
Filtration
Used to remove a solid from a liquid:f Ex: separate coffee grounds from coffee solution
Rutherford's Gold Foil Experiment
Using a block containing radioactive alpha particles, Rutherford shot these particles at a piece of gold foil which projected these deflected beams onto a circular zinc sulfide fluorescent screen. This lead to the discovery of the nucleus as some alpha particles were deflected at astonishing angles and there had to have been a denser mass in the atom.
Orbital Diagram
Using boxes to represent "building up" of atoms
Solid or liquid that is in the gaseous state
Vapor
Scientific notation
Way of writing very small or very large numbers. Consists of a coefficient, base ten and an exponent. Ex: 2.5 x 10³
zinc ion
Zn 2+
Chemical Changes (chemical reaction)
burning, combustion, corrosion, decomposition, digestion explosion, fermentation, oxidation, photosynthesis, rusting, tarnishing
Evidences of a Chemical Reaction
change in color, change in odor, production of a gas (bubbling), production of heat or light or sound, absorbing of heat or light
law of conservation of energy
energy cannot be created or destroyed only changed from one form to another
Kinetic energy
energy due to motion of molecules (chemistry)
Surroundings
everything that surrounds the system (including the thermometer!)
Millikan Experiment
found the mass of the electron.
Atomic Spectrum of Hydrogen
hv = Energy. (h = 6.63 x 10⁻³⁴J s; frequency) When hydrogen bonds absorb energy, the bonds break and become excited. Immediately, they release it as light and gives off a unique emission spectrum.
Coal
ignore
Fossil Feuls
ignore
Greenhouse effect
ignore
Infrared radiation
ignore
Natural Gas
ignore
Petroleum
ignore
Add energy to a solid and it becomes a __________
liquid (melting)
What two states of matter will flow?
liquids & gases
A (number of neutrons)
mass number
Electron Configuration
method to indicate distribution of e⁻in atom. (eg.1s²: 1st energy level, s block, 2 electrons)
Physical Change Examples
phase changes (Melting-Freezing or Boiling-Vaporizing-Condensating or sublimating-depositing); crumpling, crushing, cutting, folding, mangling, mixing, tearing, sawing, etc
Types of Solutions
solid-solid mixture ( alloys - usually two metals) solid-liquid mixture ( salt+water or sugar+water) liquid-liquid mixture (water+alcohol or water+antifreeze) gas-liquid mixture (O₂and CO₂ in seawater) gas-gas [air - N₂and O₂; scuba tank gases]
Ionic Radii
states: - cations are smaller b/c of lost outer e⁻ - anions are larger b/c of gained outer e⁻
System
the chemical or physical change that you are studying
chemical bond
the force that holds two atoms together in a molecule
Common Compounds
water (H₂O) table salt (NaCl) sucrose - sugar (C₆H₁₂O₆) carbon dioxide (CO₂) carbon monoxide (CO) ammonia (NH₃) hydrogen peroxide (H₂O₂) methane gas (CH₄)
Sublimation
when a solid changes directly to a gas (solid CO₂ turns to a vapor)