Week 1 (Intro) Flashcards
period
row in periodic table
group
column in periodic table
Alkaline Metals
group 1 of periodic table (Li, Na, K, Rb, Cs)
Alkaline earth metals
group 2 of periodic table (Be, Mg, Ca, Sr, Ba)
Halogens
group 17 of periodic table (F, Cl, Br, I, At)
Transition metals
groups 3-12 of periodic table (Sc, Co, Ni, Zn, Cu, Ag, Au, Hg, Fe)
Noble gases
group 18 of periodic table (He, Ne, Ar, Kr, Xe, Rn)
Reactivity of an element
depends on number of electrons surrounding the center, in orbitals
What is in the nucleus of an atom?
protons and neutrons
proton
positively charged particle
neutron
neutral charged particle
electron
negatively charged particle
Mass number (A)
mass of an atom, depends on number of protons and neutrons in nucleus
element
an element is a chemical substance that cannot be broken down into other substances by chemical reaction, made up of only one atom
atomic number (Z)
number of protons in nucleus of an atom, determines chemical properties of an element
Electron configuration
tells us how the electrons are arranged in the orbitals of an atom
shell
energy levels of orbitals, energy increases as distance from nucleus increases (contains subshells such as 2s, 2p)
valence electrons
occupy the outermost shell or highest energy level of an atom, participate in chemical bonding
core electrons
occupy the inner shells or lower energy levels, do not participate in chemical bonding
Main group element valence electron numbers
number of valence electrons corresponds to OLD group numbers (ex. Na has 1, B has 3, O has 6)
Noble Gas Cofiguration
8 valence electrons, a stable electron configuration that most atoms try to achieve when forming ions
How elements make ions/compounds
same group elements have similar properties
-Halogens form -1 anions (F-, Cl-, Br-, I-)
-Alkali metals form +1 cations (Li+, Na+, K+)
-Group 16 forms -2 anions (O(2-), S(2-), Se(2-))
-Alkaline Earth Metals form +2 cations (Be(2+), Mg(2+), Ca(2+))
anion
a negatively charged ion (usually nonmetals)
cation
a positively charged ion (usually metals)
ion
an atom or molecule with an electrical charge, either positive or negative
Molecular formulas
list element symbols w/ subscripts that indicate the number of atoms in the molecule, gives no info about structure (ex. CH2O)
Structural formulas
same info as molecular formula, but also show how the atoms are connected (ex. H2O->
H-O-H)
Pure substances
a single kind of matter that cannot be separated into other matter by any physical means
compound
a substance made from multiple elements
atomic element
an element with only one atom present (ex. Ne)
Molecular element
a pure substance made up of two or more atoms of the same element (ex. S8, P4, and naturally occurring diatomics: Br2, I2, N2, Cl2, H2, O2, F2)
Naturally occurring diatomics
Br2, I2, N2, Cl2, H2, O2, F2
(Brinklhof)
Molecular compounds
compounds made up of neutral elements that are held together by shared electrons via covalent bonds (ex. H2O), no polyatomic ions
Ionic compounds
neutral compounds made up of oppositely charged ions held together by an ionic bond (electron transfer) (ex. NaCl)
Ionic bond
-formed between a metal and a nonmetal (cation and anion)
-electrons are transferred
-bond is electrostatic attraction (opposite charges)
-exists as 3D lattices
Covalent bond
-formed between a nonmetal and nonmetal (neutral charges)
-electrons are shared
-exist as discrete molecules
Polyatomic Ions
covalently bonded set of two or more atoms that can behave as a single unit (can form ionic bonds with other ions) and has a net charge that is not zero
(ex. (ClO3)(-))
Conversion factors
relationships between units
in to cm
1 in = 2.54 cm
L to mL
1 L = 1000 mL
