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Chemistry (Scientific Measurement (SI prefixes (Tera (1,000,000,000,000),…
Chemistry
Scientific Measurement
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Sig Figs
measurements consists of all digits known with the uncertainty plus one final digit, somewhat uncertain or is estimated.
SI base Units
density ratio of mass to volume, or mass divided by volume
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meter, kilogram, second, kelvin, mole, ampere, candela
scientfic notation numbers are written in form m times 10n where the factor m is a greater than or equal to 1 but less than 10 and n is a whole number
Percent Error subtracting accepted value from experimental value dividing difference of the accepted value, then multiply by 100
Accuracy- closeness of a measured value to a standard or known value.
Precision- refers to the closeness of two or more measurements to each other.
Atomic Structure
History
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Dalton
5 postulates
-all matter are composed of atom -atoms of an element are identical - atoms are indivisible -atoms of diff. elements combine to form chemical compounds. -in chemical reactions atoms are rearranged.
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vocabulary
isotopes- two or more forms of the same element with different number neutrons but with same number of protons.
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average atomic mass weighted average of the atomic masses of the naturally occuring isotopes of an element
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Structure of the atom
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sub atomic particles includes protons, neutrons, electrons
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Stoichiometry
Conversions
Molar Ratio
Conversion factor that relates the amounts in moles of any two substances involved in a chemical reaction.
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Percent Yield
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Theoretical Yield- the amount you come out with when using mathmatical equations with the information you are given
chemical bonding
types
covalent bond electronegativity difference of 1.7 or less has an ionic character of 50 percent or less
non polar covalent bond a covalent bond in which the bonding electrons are shared equally by the bonded atoms
polar covalent bond a covalent bond in which the bonded atoms have an unequal attraction for the shared electrons
ionic bond a chemical bond that results from the electrostatic attraction between positive and negative ions
Lewis structures
Formulas in which atomic symbol represents nuclei inner shell electrons, dot- pairs or dashes between two atomic symbols
structural formula kind, number, arrangement, and bonds but not the unshared pairs of atoms
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The Periodic Law
structure
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blocks S-block: alkali and alkali earth metals P-block: nonmetals D-block: transition metals F-block: lanthanides and actinides
Element Groups
Alkali Metals soft, tarnish easy, low melting points, violently reactice: have 1 valence electron
alkaline Earth Metals softer than metals, react with water, 2 valence electrons, easily lose electrons
Other Metals softer than transition metals, lower boiling and melting points, electropositive
Metalloids metal & non-metal quantities, act as semiconductors, used in computer industry
nonmetals insulators or semiconductors, acidie oxides, electronegative, ionic & covalent bonds
Halogens Highly reactive: have 7 valence electrons, Toxic, Colored, poor conductors, low melting & boiling Points
Noble Gases Stable, Colorless, odorless, invert, valence shell is full
Transition Metals largest element group, hardness, high density, high melting & boiling point
Lanthanides high melting point, react with oxygen & water, dissolve in water
actinides high melting & boiling points, radioactive, artificial
Identifications
atomic radius one half the distance between two identical atoms bonded together. Period trends- gradual decrease from left to right. Group trends- increases down a group.
electronegativity: measure of the ability of an atom to attract electrons from another atom. Period trends- tends to increase across a period. Group trends- tends to decrease down a group or stay the same . Fluorine has the most electronegativity
ionization: energy required to remove one electron from a neutral atom. Period trends-generally increase across a period. Group trends- generally decreases down a group.
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Electron Cloud
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Rules/Laws
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Heisenberg Uncertainty Principle It's impossible to determine simultaneously both the position and velocity of an electron or any other particle
Hund's Rule orbitals of equal energy are each occupied by 1 electron before any orbital is occupied by a second
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