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109 Cards in this Set
- Front
- Back
Chemistry is the study of matter
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its compositions, properties, and transformations
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Matter is
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anything that has mass and takes up volume
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Physical properties are those
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that can be observed or measured without changing the composition of the material
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Chemical properties are those
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that how a substance can be converted to another substance
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Pure substance
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is composed of a single component and has a constant composition, regardless of the sample size and the origin of the sample
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A Mixture
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is composed of more then one component. The composition of a mixture can vary depending on the sample
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An element
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is a pure substance that cannot be broken down into a simpler substances by a chemical reaction
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a compound
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is a pure substance formed by by chemically combining (joining together) two or more elements
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Every measurement
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is composed of a number and a unit
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Metric measurement Length
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Meter
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Metric Measurement Mass
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gram
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Metric Measurement Volume
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Liter
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Time
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Second
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Mega
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Million
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Kilo
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Thousand
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deci
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tenth
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Centi
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Hundreth
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Milli
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Thousand
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Micro
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Millionth u
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One milliliter
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is the same as one cubic centimeter (cm3) which is abbreviated as cc
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Numbers in chemistry are
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inexact or exact
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An exact number
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results from counting objects or is part of a definition
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An inexact number
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results from a measurement or observation and contains some uncertainty
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1qt=
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946mL
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1fl oz =
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29.6mL
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1in=
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2.54cm
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1m=
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39.4in
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1km=
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0.621 mi
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1kg=
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2.21Lb
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454g=
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1Lb
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28.4g=
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1oz.
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Significant number in Multiplication and Division
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the answer has the same number of significant figures as the original number with the fewest significant digits
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Significant number in addition and subtraction
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the answer has the same number of decimal places as the original number with the fewest decimal places.
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Convert Fahrenheit to Celsius
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F=1.8(c) +32
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Convert Celsius to Fahrenheit
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C= F-32/1.8
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convert Kelvin to Celsius
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K= C + 273
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Convert Celsius to Kelvin
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C = K-273
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Density
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is the physical property that relates the mass of a substance to its volume
density= mass(g)/volume (mL or cc) |
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An element
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is a pure substance that cannot be broken down into simpler substances by a chemical reaction
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Metals are
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shiny solids that are good conductors of heat and electricity. all metals are solid at room temperature except for mercury which is liquid
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Nonmetals
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do not have a shiny appearance and they are generally poor conductors of heat and electricity. Nonmetals are sulfur,carbon nitrogen oxygen bromine (liquid at room temperature) 9 others
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Metalloids
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have properties intermediate between metals and nonmetals only 7 elements a metalloids=boron, silicon,germanium,arsenic, antimony, tellurium, and Astatine
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Four nonmetals
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compromise 96% of the human body Oxygen, carbon, hydrogen, and nitrogen
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Major minerals or Macronutrients
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Sodium, Potassium and chlorine Magnesium and sulfur Calcium and Phosphorus
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Trace elements or micronutrients
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iron,zinc iodine, fluorine, and selenium
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A Chemical formula
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uses element symbols to show the identity of the elements forming a compound and subscripts to show the ratio of atoms (the building blocks of matter) contained in the compound
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A Proton
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symbolized by p, has a positive charge
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An electron
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symbolized by e", has a negative charge
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A neutron
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symbolized by n, has no charge
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All matter is composed of
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basic building blocks called atoms
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The nucleus of an atom
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contains the protons and neutrons of the atom
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The electron cloud is
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composed of electrons
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Mass number symbolized by A
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the number of protons and neutrons in the atom (element)
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Atomic number (Z)
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is the number of protons in the atom
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Isotopes are atoms
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of the same element (number of protons) with a different number of neutrons
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118Sn
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mass weight 118 of element Tin
50 is the protons therefore their are 68nuetrons in this isotope. |
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A row in the periodic table is called
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a period similar in size there are 7
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a column in the periodic table is called
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a group elements in a group have similar electronic and chemical properties
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Alkali metals are
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group 1a
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Alkaline Earth elements are
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group 2a
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Halogens are
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group 7a
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Noble gases are
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group 8a
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Shell 1 holds
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2 electrons
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Shell 2 holds
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8 electrons 2s 2p 2p 2p
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Shell 3 holds
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18 electrons
3s, 2 3p,3p,3p, 6 3d,3d,3d,3d,3d 10 |
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Shell 4 holds
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32 electrons
4s 2 4p,4p,4p 6 4d,4d,4d,4d,4d, 10 4f,4f,4f,4f,4f,4f,4f, 14 |
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each orbital hold a max of
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2 electrons
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Electron dot symbol
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carbon has 4 electrons
. .C. . |
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The size of atoms increases
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down a column
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The size of atoms decreases
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across the row therefore helium is smallest and Francium is largest
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Bonding
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is the joining of two atoms in a stable arrangement
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Ionic bonds
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result from the transfer of electrons from one element to another
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covalent bonds
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result from sharing of electrons between two atoms
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Ionic bonds form between a
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metal on the left side of the periodic table and a nonmetal on the right
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ions
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charges species in which the number of protons and electrons in an atom is not equal
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A molecule
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is a discrete group of atoms that share electrons
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Covalent bonds are
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when two nonmetals combine, or when a metalliod bonds to a non metal
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Cations are
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postively charged ions has fewer electrons than protons
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anions are
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negatively charged ions has more electrons then protons
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metals form
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cations by losing one two or three electrons we show this by + smybol
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Nonmetals form
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anions by gaining one, two, three, electrons we symbolize this by using -
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Ionic compounds are composed of
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cations and anions
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The sum of the charges in an ionic compound is
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zero
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ous
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is the smaller charge example Fe2+ is iron II or ferrous
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ic
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is for the higher charge example Fe3+ is Iron III or ferric
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Anions are named by replacing the ending with
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ide example chlorine is chloride
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Name the cation and then the anion
example Na+ F- |
sodium floride
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Cu+
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Cuprous
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Cu2+
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Cupric
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Cr2+
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Chromous
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Cr3+
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Chromic
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Fe2+
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ferrous
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Fe3+
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ferric
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Sn2+
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Stannous
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Sn4+
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Stannic
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CO3 2-
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Carbonate
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HCO3 -
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hydrogen carbonate or bicarbonate
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CH3CO2 -
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Acetate
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-CN
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Cyanide
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NO3 -
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Nitrate
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NO2 -
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Nitrite
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-OH
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Hydroxide
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PO4 3-
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Phosphate
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HPO4 -
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Hydrogen phosphate
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H2PO4 -
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Di-hydrogen phosphate
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SO4 2-
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Sulfate
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HSO4 -
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Hydrogen sulfate
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SO3 2-
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Sulfite
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HSO3 -
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Hydrogen sulfite
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