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168 Cards in this Set
- Front
- Back
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Matter
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Anything that occupies space and has mass.
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States of Matter
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Solid Liquid Gas
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Solid Matter has _____ KE and ______ compressibility
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low / low
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Liquid Matter has _____ KE and _____ compressibility
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medium / low
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Gas Matter has _____ KE and ____ compressibility
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high / high
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Elements
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composed of only one type of atom; cannot be separated into simpler substances by chemical means
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Compounds
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composed of atoms of two or more elements; NOT a mixture of different elements
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Name 2 key properties of compounds
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DISTINCT properties
DEFINITE composition |
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What is the difference between a mixture and a pure substance?
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Mixtures can be separated by physical methods into pure substances
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What is the difference between mixtures and compounds?
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Mixtures are pure substances in varying ratios. Compounds are atoms of 2 or more elements with DISTINCT properties and DEFINITE composition
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What is the difference between elements and compounds?
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Elements are pure substances, compounds are 2 or more elements joined together
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Homogeneous Mixture
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The same throughout
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Heterogeneous Mixture
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Not the same throughout, cookies or vegetable soup
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What method is used to separate a compound?
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Chemical
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What method is used to separate a Mixture?
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Physical
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Physical Property
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A characteristic that can be observed or measured without changing the identity of the substance (Length, odor, color, size, density, MP, BP)
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Chemical Property
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Describes the ability of a substance to undergo changes that alter its identity
(The ability of coal to burn and iron to rust) |
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Density =
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Mass
-------- Volume |
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Volume =
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Mass
--------- Density |
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Mass =
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Volume x Density
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Three units of measure for temperature
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C, F, K
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Formula for converting Celsius to Kelvin
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Tk= 273.15 + Tc
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Formula for Converting Celsius to Farenheit
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Tf= 32.0 + (9/5)Tc
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Extensive property
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External property, depends on how much matter present
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Intensive Property
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Internal property, independant of amount of matter
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Physical Change
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When a substance changes physical condition but does not involve a change in composition
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Chemical Change
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When a substance changes into another substance or group of substances
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SI Units
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Metric System, based on powers of 10
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Common SI unit for Mass
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Kilogram
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Common SI unit for Length
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Meter
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Common SI unit for Volume
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m^3
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Kilo-
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one thousand 10^3
(move decimal 3 to the right) |
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Centi-
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one hundredTH 10^-2
(Move decimal 2 to the left) |
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milli-
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one thousandTH 10^-3
(move decimal 3 to the left) |
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deci-
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tenth 10^-1
(move decimal 1 to the left) |
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Conversion Factor
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Express the equivalence of measurement in two different units. It is always written as a fractrion, usually new/old
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Accuracy
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Whether the measurement is correct, how close the result is to the accepted value
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Precision
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How much uncertainty is associated wiht the measurement, how closely different measurements of the same object agree with one another
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Significant Figures
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Meaningful digits in a measured or calculated quantity: Certain Digits plus One Uncertain (rounded) digit
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Rules for adding and subtracting sig figs
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Answer cannot have more places after the decimal point than either of the original figures.
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Rules for dividing/multiplying sig figs
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Answer cannot have more total sig figs than either of the original figures
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Order of operations for Sig Figs
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Track the significant figures using the appropriate rule for each step, but don't round off till the end.
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Scientific Notation
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N x 10^n
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4 Points of Daltons Atomic Theory
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-An element is made up of atoms. All atoms are identical
-Atoms cannot be destroyed or created -All atoms of one element have the same size, mass, and property. Atoms of two different elements have different sizes, masses, and properties -Atoms of different elements may combine in simple, whole-number ratios to form compounds |
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2 points of Dalton's Atomic Theory were disproved. What discoveries disproved them?
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Isotopes- Atoms of the same element are NOT identical
Subatomic Particles: atoms are NOT indivisible |
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2 points of Dalton's Atomic Theory are now Laws. What are they called?
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Law of Conservation of Matter
Law of Constant composition |
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Three Subatomic Particles and their symbol/charge
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Proton p+ +1
Neutron n 0 Electron e- -1 |
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Atoms are mostly _____
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empty space
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The nucleus is made up of _____
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protons and neutrons
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______ are found outside of the nucleus of the atom
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electrons
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______ makes up most of the mass of an atom
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The nucleus
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Atomic number =
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(Z) Number of protons
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Mass Number =
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(A) number of protons + number of neutrons
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Atomic Mass Unit
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(amu) 1 amu = 1/12 of the mass of an atom of C with 6 protons and 6 neutrons. Such a C atom has a mass of 12amu
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Conversion Factor for amu to g
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1 amu = 1.661 x 10^(-24)g
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Mass of a Proton
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1.672623 x 10^(-24)g
1.007 amu |
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Mass of a Neutron
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1.674286 x 10^(-24)g
1.009 amu |
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Mass of an Electron
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0.109389 x 10^(-26)g
.0005amu |
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Rutherford Experiment
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A narrow beam of positively charged (alpha) (+2) particles was directed at a very thin gold foil. Most particles past through, Few were deflected at moderate angles, and very few were deflected at acute angles. Some positive particles were deflected by coming to close to a + charged nucleus, some collided with a nucleus and were repelled backward
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Isotopes
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atoms with the same atomic number (Z) but different mass number (A). atoms of the same elements that differ in the number of neutrons
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%Abundance of Isotopes =
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(#number of atoms of a given isotope)
------------------------------------------- total # of atoms of all isotopes of that element all times 100% |
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Average atomic mass =
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n
sum (abund. N x mass N) n=1 |
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Periodic Table
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A visual summary of all the elements and some of their similarities to each other.
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2 specific ways the periodic table is organized:
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Increasing Atomic Number
Similar Chemical/Physical properties |
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Groups or Families
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vertical columns numbered 1 to 8 with each number followed by A or B, elements in the same GROUP have similar chem/phys properties
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A Groups
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Main Elements
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B Groups
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Transition Elements
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Periods
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Horizontal rows numbered 1-7
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properties of Metals
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-lustrous appearance
-maleable -electric and thermal conductors -tend to form (+) ions in ionic compounds |
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Properties of Non-Metals
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-dull appearance
-wide diversity in physical states with solids being brittle or soft -poor electrical and thermal conductors -tend to form (-) ions in ionic compounds |
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Periodic table can be easily separated into these 3 sections
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Metals, Non-Metals, Metalloids
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Group 1A
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Alkali Metals (not H). React strongly with water to produce hydrogen gas and alkaline solutions. Only found as parts of compounds, never as free elements
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Group 2A
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Alkaline Earth Metals: Elements (Except Be) and their oxides react with water to form alkaline solutions
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Group 7A
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Halogens: Non-metals that are extremely reactive with alkali metals to form salts. Reactive elements that generally exist in their elemental form as diatomic molecules
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Group 8A
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Noble Gases: Least reactive elements, very low abundance on earth.
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Group B
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Transition elements/ transition metals: Contain some of the most useful and abundant elements.
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Actinides and Lanthanides
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Groub B metals, contain well-known radioactive elements such as U, Pu
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Compounds
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A combination of 2 or more elements in definite ratios by mass
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Molecule
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The smalles unit of a molecular compound that retains the characteristics of the compound
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Chemical formulas
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Symbols used to describe the composition of compounds
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A subscript in a chemical formula represents:
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The number atoms for that element: H2O = 2 hydrogen and 1 oxygen
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7 Diatomic Elements and their Formulas
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H2, N2, O2, F2, Cl2, Br2, I2
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Ions
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atoms (monatomic) or groups of atoms (polyatomic) with a positive or negative charge; ions are the smalles formula units to describe ionic compounds
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Cation
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positively charged ion. Metals generally lose electrons during a reaction to form cations.
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Anion
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negatively charged ion. Nonmetals frequently gain electrions to form anions
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Rules for determining charges on ions
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Main group metals: (+) charge number = group number (1,2,3)
Main group nonmetals: (-) charge number = group number -8 Transition elements generally have +2 or +3 charges |
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Polyatomic Ions
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Groups of ions that bear a net charge
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Ionic compounds
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Cations + Anions
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Formula for writing ionic coumpounds
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Cation Anion
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All ionic compounds must have a net ______ charge
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neutral
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Coulomb's Law
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The oppositely charged ions are attracted to each other by electrostatic forces
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Rules for electrostatic attraction
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As charge increases and size decreases, attraction increases.
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The two types of compounds
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Molecular and Ionic
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Molecular compounds can only be made up of:
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nonmetals and metaloids
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Ionic compounds are made up of
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Metals and nonmetals
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Binary Molecular compounds are made up of
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TWO types of non-metals
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Rules for naming a binary molecular compound:
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(prefix)1st element +
(prefix)2nd elementIDE |
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H(2)O
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Water
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NH(3)
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Ammonia
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Rules for naming Cations with one possible charge
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name + ion
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Rules for naming cations with multiple possible charges
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name (roman numeral) ion
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NH(4)+
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Ammonium Ion
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Rules for Naming Monatomic Anions
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rootname + ide
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Rules for Naming Ionic Compounds
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-NO NUMBER PREFIXES!
-Cation + AnionIDE (Same rules for each monatomic ion) -Charges must balance |
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Oxoanions
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Polyatomic anions containing oxygen
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Rules for Naming Oxoanions with 1 possible charge
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anion-ate
-Groups IIIA and IV A |
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Rules for naming Oxoanions with 2 possible charges
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more oxygen -ate
less oxygen -ite Groups V A and VI A |
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Rules for naming Oxoanions with 4 possible charges
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1- hypo____ite
2- ____ite 3- ____ate 4- per_____ate Group VII A |
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Hydrate
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ionic compoun that carries a definite number of water molecules along in the crystal structure
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The water in a hydrate is called
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Water of Hydration
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How to determine the chemical formula of a hydrate
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Heat the sample and measure the weight loss, which is the weight of water in the hydrate
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Formula for a hydrate
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formula for an anhydrous compound + (DOT) + number of water molecules in the hydrate
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Acid
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a molecular compound that dissociates in water to give a hydrogen ion H+ and an anion
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Monoprotic Acid
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one acid molecule only releases one proton H+
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Polyprotic Acid
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one acid molecule can release more than one proton H+
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Rules for naming acid are based on
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the prefixes and suffixes of the anion
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If the prefix/suffix of the anion was -ide, the acid will be named
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hydro_____ic acid
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If the prefix/suffix of the anion was per____ate, the acid will be named
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per_____ic acid
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If the prefix/suffix of the anion was -ate, the acid will be named
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_______ic acid
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If the prefix/suffix of the anion was -ite, the acid will be named
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____ous acid
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If the prefix/suffix of the acid was hypo____ite, the acid will be named
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hypo____ous acid
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Is HCl hydrochloric acid or hydrogen chloride?
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Depends on if it is gas (g) or an aqueous solution (aq)
HCl (g) hydrogen chloride HCl (aq) hydrochloric acid |
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HC(2)H(3)O(2)
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Acetic Acid
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C(2)H(3)O(2)
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Acetate Ion
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HI (g)
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hydrogen iodide
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HI (aq)
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hydroiodic acid
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HCN
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hydrocyanic acid
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CN-
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cyanide ion
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NH(4)+
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Ammonium ion
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OH-
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Hydroxide ion (gives the property of a base)
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HCO(3)
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Bicarbonate (or hydrogen carbonate) ion
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CrO(4)2-
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Cromate ion
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Cr(2)O(7)2-
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dicromate ion
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MnO(4)-
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Permanganate ion
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How do we connect the macroscopic world we're dealing with to the particulate world of atoms and molecules?
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Mole and Molar Mass
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Mole
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SI Unit for amount of substance
(the # of C-12 atmons in exactly 12g of C-12 = 12amu) |
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1 mol of any substance =
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6.022 x 10^(23) units
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Avagadro's Number
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6.0221415 x 10^(23)
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Molar Mass
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the mass in grams of 1 mole of a substance
and the mass in grams of 6.02 x 10^(23) particles of that substance |
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Molar Mass =
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Mass g
_____ = _______ Mole mol |
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Atomic Weight reported in the Periodic Table can be used in what two units?
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-Atomic Mass Unit: Mass of one atom (amu/atom)
-Molar Mass: Mass of one mole of atoms (g/mol) |
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What is the formula to convert Moles to Mass?
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grams
Moles x ---------=grams 1mol |
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What is the formula to convert mass to moles?
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1 mol
grams x ---------- = moles grams where grams = 1 / molar mass |
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Molecular Weight (in amu)
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the sum of the atomic weights of all atoms in one molecule;
molar mass of a compound - molecular weight in grams |
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CO(3)2-
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carbonate ion
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NO(2)-
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nitrite ion
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NO(3)-
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nitrate
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PO(4)3-
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phosphate ion
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HPO(4)2-
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hydrogen phosphate ion
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H(2)PO(4)
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dihydrogen phosphate
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OH-
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hydroxide ion
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SO(3)2-
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sulfite ion
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SO(4)2-
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sulfate
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HSO(4)-
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hydrogen sulfate ion
(or bisulfate ion) |
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ClO-
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hypochlorite ion
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ClO(2)-
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chlorite ion
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ClO(3)-
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chlorate ion
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ClO(4)-
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perchlorate ion
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CrO(4)2-
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chromate ion
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Cr(2)O(7)2-
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dichromate ion
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MnO(4)-
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permanganate
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Name the Ions with more than one possible charge
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Chromium, manganese, iron, cobalt, copper, mercury, tin, lead
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PO(4)3-
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phosphate
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PO(3)3-
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phosphite
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HPO(4)2-
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hydrogen phosphate
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O(2)2-
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peroxide
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SCN-
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thiocyanate
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percent composition
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expressed as the percent (by mass) of each element in a compound
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