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46 Cards in this Set
- Front
- Back
Atoms
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make up all matter, elements
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Subatomic particles
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protons, neutrons, electrons
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Protons
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positively charged, in nucleus
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Neutron
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no charge, in nucleus
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Electron
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negatively charged, in electron cloud
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Atomic number
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number of protons in an atom, defines the atom, same element=same atomic number
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Mass number
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number of protons and neutrons in an atom, can be different for same element
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Chemical formula
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Mass number= top left
Atomic number= bottom left Charge= top right # of atoms= bottom right |
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Ion
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charged particle
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Isotopes
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Atom w/ same number of protons, but different number of neutrons... different mass number
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Mole
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6.022*10^23
unit to measure the number of particles of a substance Avogadro's number |
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Average atomic mass
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how many g/mol
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Dmitri Mendeleev
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first periodic table, by mass number, patterns in physical and chemical properties
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Henry Mosley
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solved Mendeleev's problems, increased by atomic number (protons), current table
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Periodic Law
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patterns seen when elements are arranged by increasing atomic number
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Group (Family)
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Vertical column, elemeents have similar properties
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Period
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horizontal row, elements don't have similar properties, get less reactive from left to right
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Alkali Metals
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Group 1, highly reactive, not including hydrogen
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Alkaline Earth Metals
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Group 2
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Halogens
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Group 17
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Nobel Gases
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Group 18
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Main Group Elements
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s and p orbitals, groups 1-2 and 13-18
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Transition Elements
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d orbitals, groups 3-12
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Lanthanides
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elements 58-71
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Actinides
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Elements 90-103
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Metalloids
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Adjacent to red line, not Al
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Non-metals
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right of red line and H
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Metals
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left of red line, not H
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Atomic Raduis
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measurement of the size of an atom
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AR Period Trend
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decreases moving left to right, as element gains electron in same energy level, electrons pulled tighter
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AR Group Trend
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increases moving down a group, electrons farther from nucleus and eachother
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Ionization
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losing an electron
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Cation
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ion w/ positive charge, metals lose electrons, less electrons-less repulsion, become smaller
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Ionization Energy
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energy needed to remove an electron from a neutral atom
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I periodic trend
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Ionization energy increases moving left to right
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I group trend
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Ionization energy decreases moving down a group
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Electron Affinity
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energy change observed when an atom gains an electron
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EA periodic trend
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increases moving left to right, greater distance it can travel, increased energy
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EA group trend
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decreases moving down a group, less distance to travel
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Electronegativity
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ability to pull an electron towards the nucleus
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EN periodic trend
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increases moving left to right
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EN group trend
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decreases moving down a group
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Ionic Radius
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measurement of the size of an ion
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Anion
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Non-metals gain electrons, more electrons- electron repulsion, become bigger
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IR periodic trend
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increases moving left to right, anions are on the right side
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IR group trend
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increases moving down a group, more electron orbitals
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