Chapters 11&12: Atomic Theory and The Periodic Table Flashcards
Electrons
the negatively charged particles in an atom
Atom
the smallest particle in which an element can be divided and still be the same substance
Protons
the positively charged particles in the nucleus
Neutrons
the particles of the nucleus that have no charge
Nucleus
the center of the atom that is a tiny, extremely dense, positively charged part of the nucleus
Electron cloud
region in the atom where electrons are likely to be found
Atomic mass unit (amu)
the SI unit used to express the masses of particles in atoms
Atomic Number
the number of protons (or electrons) in an atom
determines the identity of an element
every element has a unique atomic number
Isotopes
atoms that have the same number of protons but have different number of neutrons
Mass number
the sum of the protons and neutrons in an atom
Atomic mass
the weighted average of the masses of all the naturally occurring isotopes
Periodic
happening at regular intervals
Periodic Law
the chemical and physical properties of the elements repeat periodically when the elements are lined up by their atomic numbers
Metals
shiny ductile- drawn into thin wires good conductors of electric current malleable- can be flattened with a hammer good conductors of thermal energy
Metals (Periodic Table)
left of the zigzag line
Nonmetals
not malleable or ductile not shiny poor conductors of thermal energy and electric current (opposite of metal) brittle
Nonmetals (Periodic Table)
right of the zigzag line
Metalloids (semiconductors)
shiny
brittle- easily smashed
hard but brittle
good conductor of electric current
Metalloids (Periodic Table)
border the zigzag line
Period/Series
horizontal row of elements on the periodic table
same number if principle energy levels
Group/Family
vertical column of elements on the periodic table
Energy levels
a layer of electrons
Farther from nucleus= ______
nearest= ___ energy level; ___ energy
farther out= ____ energy level; _____ energy
more energy
1st; most energy
2nd; less energy
Valence electron
electron on the outermost or highest energy level
Ion
an atom or group of atoms with a net(sum) positive or negative charge, depends on gaining or losing electrons
Cation
positive ion, more protons than electrons so had to lose some electrons
Anion
negative ion, more electrons than protons so had to gain electrons
Octet rule
atoms tend to gain, lose, or share electrons in order to acquire the electron structure of the nearest noble gas (18th column)
Alkali
the first group in the periodic table lose 1 electron ion: 1+ has 1 electron in its outermost energy level most reactive metals
Alkaline earth
the second group in the periodic table
lose 2 electrons
ion: 2+
Transition elements
groups 3-12 in the periodic table
Halogens
the seventeenth group in the periodic table
gain 1 electron
ion: 1-
Noble gases (periodic table)
the eighteenth group in the periodic table
doesn’t gain, share, or lose electrons (octet present)
full set of electrons in its outermost energy level
unreactive elements
Inner transition elements
Both rows on the bottom of the periodic table
Rare earth elements
1st row of the blocks on the bottom of the periodic table
Solid
the state of matter in which the volume and shape of a substance are fixed
Liquid
the state of matter that has a definite volume but not a definite shape
Gas
the state of matter does not have a definite volume or shape
Luster
when a substance is shiny
Conductor
when a substance conducts heat or electricity well
Insulator
when a substance does not conduct heat or electricity well
Ductile
when a substance can be drawn or extruded into a wire
Malleable
when a substance can be rolled or pounded into thin sheets
Brittle
when a substance breaks, it crumbles
Noble gases
colorless
odorless
gases
Group 13
lose 3 electrons
3+
Group 14
share electrons only
Group 15
gain 3 electrons or share
3-
Group 16
gain 2 electrons or share
2-
Group 17
gain 1 electron or share
1-
Monotomic ions
ions made from one atom
Nonmetals (list elements)
nitrogen (N) sulfur (S) oxygen (O) selenium (Se) fluorine (Fl) bromine (Br) phosphorus (P) iodine (I) chloride (Cl)
Metalloids (list elements)
boron (B) arsenic (As)
aluminum (Al) antimony (Sb)
silicon (Si) tellurium (Te)
germanium (Ge) polonium (Po)
Cation (rule for naming)
(metals)
take the name of the parent atom (same name)
ex. aluminum
Anions (rule for naming)
(nonmetals)
change the name of the parent atom to “ide”
ex. nitride
Anion names
nitride sulfide oxide selenide fluoride bromide phosphide iodide chloride
Atomic mass equation
( # of element x % of element) =
( # of element x % of element) =______add together
__ amu
Mendeleev’s periodic table
allowed for the prediction of the properties of the missing elements
