Chemistry - Mr Larry - Final Notes
ammonium carbonate
(NH₄)₂CO₃
high
*describe this property in an ionic compound* boiling point
brittle
*describe this property in an ionic compound* brittleness
good
*describe this property in an ionic compound* electrical conductivity in the liquid state
poor
*describe this property in an ionic compound* electrical conductivity in the solid state
good
*describe this property in an ionic compound* electrical conductivity when dissolved in water
hard
*describe this property in an ionic compound* hardness
high
*describe this property in an ionic compound* melting point
no
*for each statement, write yes if evidence of a chemical reaction is present. write no if there is no evidence of a chemical reaction* a drinking glass breaks into smaller pieces
no
*for each statement, write yes if evidence of a chemical reaction is present. write no if there is no evidence of a chemical reaction* a piece of ice melts
yes
*for each statement, write yes if evidence of a chemical reaction is present. write no if there is no evidence of a chemical reaction* a tomato smells rotten
yes
*for each statement, write yes if evidence of a chemical reaction is present. write no if there is no evidence of a chemical reaction* baking powder produces a gas that makes a cake rise
yes
*for each statement, write yes if evidence of a chemical reaction is present. write no if there is no evidence of a chemical reaction* candle wax burns
yes
*for each statement, write yes if evidence of a chemical reaction is present. write no if there is no evidence of a chemical reaction* drain cleaner is mixed with water and the solution becomes warm
yes
*for each statement, write yes if evidence of a chemical reaction is present. write no if there is no evidence of a chemical reaction* green leaves turn yellow and red as the seasons change
no
*for each statement, write yes if evidence of a chemical reaction is present. write no if there is no evidence of a chemical reaction* molten candle wax solidifies
Cs₂SO₄(l) + H₂O(l) (water)
*predict the products for each reaction. write the formulas for these products on the product side of each equation. then indicate what type of product is produced during the reaction shown in precipitates* CsOH(aq) + H₂SO₄(aq) → ___+____
KBr + H₂O (water)
*predict the products for each reaction. write the formulas for these products on the product side of each equation. then indicate what type of product is produced during the reaction shown in precipitates* HBr(aq) + KOH(aq) → ___ + ___
2KCl(g) + H₂S(g) (gas)
*predict the products for each reaction. write the formulas for these products on the product side of each equation. then indicate what type of product is produced during the reaction shown in precipitates* K₂S(aq) + HCl(aq) → __+__
Exothermic
- gas to liquid to solid - energy is released - bomb - burning anything - making ice cream - anything that emits light
ionic
- nonmetal/metal - transfers electrons - has polyatomic - has roman numerals
covalent
- shares electrons - nonmetal/nonmetal - uses prefixes - double covalent bond - 4
Endothermic
- solid to liquid to gas - energy taken in - snow melting - baking anything (bread) - water/perspiration evaporates
synthesis reaction
2 or more substances -> 1 compound
Hydrate
A compound that has a specific number of water molecules bound to its atoms
Period
A horizontal row of elements in the modern periodic table; series
anion
A negatively charged ion
silver nitrate
AgNO₃
Transition elements
An element in groups 3-12 of the modern periodic table and further divided into transition metals and inner transition metals
Electrolyte
An ionic compound whose aqueous solution conducts an electric current
bromine chloride
BrCl
methane
CH₄
carbon monoxide
CO
carbon dioxide
CO₂
calcium oxalate
CaC₂O₄
calcium hydride
CaH₂
chlorine trifluoride
ClF₃
chromium(II) hydroxide
Cr(OH)₂
2, 2
Cu(NO₃)₂(aq) + __ NaOH(aq) → Cu(OH)₂(s) + __ NaNO₃(aq)
copper(I) chloride
CuCl
5, 3, 4
C₃H₈(g) + __ O₂(g) →__ CO₂(g) + __ H₂O(g)
iron(II) nitrate
Fe(NO₃)₂
fluorine
F₂
(g)
Gas
Alkali metal
Group 1 elements, except for hydrogen, they are reactive and usually exist as compounds with other elements
hydrobromic acid
HBr
bromic acid
HBrO₃
nitrous acid
HNO₂
nitric acid
HNO₃
mercury(II) nitrate
Hg(NO₃)₂
mercury(I) chloride
Hg₂Cl₂
carbonic acid
H₂CO₃
bent
H₂O
water
H₂O
3, 3
H₃PO₄(aq) + __ KOH(aq) → __ H₂O(l) + K₃PO₄(aq)
potassium cyanide
KCN
potassium sodium carbonate
KNaCO₃
lithium acetate
LiCH₃COO
(l)
Liquid
magnesium hydroxide
Mg(OH)₂
nitrogen trichloride
NCl₃
nitrogen trifluoride
NF₃
ammonia
NH₃
amonia
NH₃
ammonium acetate
NH₄CH₃COO
nitrogen monoxide
NO
sodium dihydrogen phosphate
NaH₂PO₄
sodium phosphate
Na₃PO₄
trigonal bipyramidal
NbBr₅
nickel(II) nitrate
Ni(NO₃)₂
dinitrogen tetroxide
N₂O₄
oxygen dibromide
OBr₂
lead (II) chloride
PbCl₂
diphosphorus pentoxide
P₂O₅
single-replacement reaction
Q + XZ → X + QZ
synthesis reaction
Q + Z → QZ
double replacement reaction
QT + XZ → QZ + XT
decomposition reaction
QT → Q + T
sulfur tetrachloride
SCl₄
Selenium tetrachloride
SeCl₄
tin(IV) nitrate
Sn(NO₃)₄
(s)
Solid
strontium nitrate
Sr(NO₃)₂
16, 8
S₈(s) + ___ Cu(s) → ___ Cu₂S(s)
tellurium tetrabromide
TeBr₄
tellurium diiodide
TeI₂
Formula unit
The simplest ratio of ions represented in an ionic compound
Group
Vertical column of elements in the periodic table; arranged by increasing atomic number; families
(aq)
Water solution
zinc chlorate
Zn(ClO₃)₂
2, 2
__ SO₂(g) + O₂(g) → __ SO₃(g)
2, 3, 2
___ Al(s) + ____ Cl₂(g) → ___ AlCl₃
ionic
___ compounds are generally composed of a metal and a nonmetal
nitrate
___ is an example of an ion that forms resonance structures (more than one structural formula)
Crystal lattice
a 3-dimensional geometric arrangement of particles in which each positive ion is surrounded by negative ions and each negative ion is surrounded by positive ions; vary in shape due to sizes and relative numbers of the ions bonded
anion
a Cl⁻ ion is an example of a ____
binary compound
a ___ contains only two elements
subscript
a ___ is a small number used to represent the number of ions of a given element in a chemical formula
structural formula
a ___ shows the arrangement of the atoms in a molecule
Pi bond
a bond that is formed when parallel orbitals overlap to share electrons
Covalent bond
a bond that results from the sharing of valence electrons
Synthesis reaction
a chemical reaction in which two or more substances react to yield a single product
Endothermic
a chemical reaction or process in which a greater amount of energy is required to break the existing bonds in the reactants than is released when the new bonds form in the product molecules
Exothermic
a chemical reaction or process in which more energy is released than is required to break bonds in the initial reactants
Double replacement reaction
a chemical reaction that involves the exchange of ions between two compounds and produces either a precipitate, a gas, or water ex) compound + compound -> 1-2 compounds
Decomposition reaction
a chemical reaction that occurs when a single compound breaks down into two or more elements or new compounds
Single replacement reaction
a chemical reaction that occurs when the atoms of one element replace the atoms of another element in a compound
ionic bond
a force that holds together atoms that are oppositely charged
Halogen
a highly reactive group 17 element
Alloy
a mixture of elements that has metallic properties; most commonly forms when the elements are either similar in size (substitutional alloy) or the atoms of one element are much smaller then the atoms of another (interstitial)
Lewis structure
a model that uses electron-dot structures to show how electrons are arranged in molecules. pairs of dots or lines represent bonding pairs
VSEPR (valence shell electron pair repulsion) model
a model used to determine molecular shape
Structural formula
a molecular model that uses symbols and bonds to show relative positions of atoms; can be predicted for many molecules by drawing the Lewis structure
monatomic
a one-atom ion is called a ___ ion
Oxyanion
a polyatomic ion composed of an element, usually a nonmetal, bonded to one or more oxygen atoms
cation
a positively charged ion is called a ___
Hybridization
a process in which atomic orbitals are mixed to form new, identical hybrid orbitals
Precipitate
a solid produced during a chemical reaction in a solution
Aqueous solution
a solution in which the solvent is water
Reactant
a starting substance in a chemical reaction
Chemical equation
a statement using chemical formulas to describe the identities and relative amounts of the reactants and products involved in the chemical reaction ex) 2 Fe(s) + 3Cl₂(g) -> 2FeCl₃ (s)
Product
a substance that forms in a chemical reaction
Polar covalent bond
a type of bond that forms when electrons are not shared equally
Inner transition metal
a type of group B element that is contained in the f-block of the beriodic table and is characterized by a filled outermost orbital and filled or partially filled 4f and 5f orbitals
activity
ability of an element to react
salt + water NaCl + H₂O
acid + base → ___+___ HCl + NaOH →___+___
metallic oxide + water SO₃ + H₂O
acid →___+___ H₂SO₄ →___ +___
metal compound + hydrogen MgCl₂ + H₂
active metal + acid → ___+___ Mg + 2HCl
Al(NO₃)₃
aluminum nitrate
(NH₄)₂Cr₂O₇
ammonium dichromate
Bond dissociation
amount of energy to break a specific bond (hydrogen is the easiest bond to break)
Ion
an atom or bonded group of atoms with a positive or negative charge
Metal
an element that is solid at room temperature, a good conductor of heat and electricity, and generally is shiny; most metals are ductile and malleable
Noble gas
an extremely unreactive group 18 element
Anion
an ion with a negative charge
Cation
an ion with a positive charge
Net ionic equation
an ionic equation that includes only the particles that participate in the reaction
Complete ionic equation
an ionic equation that shows all the particles in a solution as they realistically exist
Oxyacid
any acid that contains hydrogen and an oxyanion (any acid that contains oxygen) ex.) H₂SO₄
BaBr₂
barium bromide
the nuclei of two attached atoms
bond length is the distance between ____
CdSO₄
cadmium sulfate
Ca + H₂O → CaO + H₂
calcium and water
CaBr₂
calcium bromide
CaO
calcium oxide
CS₂
carbon disulfide
CI₄
carbon tetraiodide
Polyatomic ion
charged particle containing more than one atom
Monatomic ion
charged particle containing only one atom
Periodic law
chart that organizes all known elements into a grid of horizontial rows (periods), and vertical columns (groups/families) arranged by increasing atomic number
catalyst
chemical formula written over the arrow in a chemical equation signifies a ___ for the reaction
CrBr₃
chromium(III) bromide
metal + oxygen → metal oxide nonmetal + oxygen → nonmetal oxide compound + oxygen → 2 or more oxides CH₄ + 2O₂ → CO₂ + 2H₂O S + O₂ → SO₂
combustion reaction
Ionic compound
compounds that contain ionic bonds
Resonance
condition that occurs when more than one valid Lewis structure exists for the same molecule
electrolysis
decomposition of a substance by an electric current (separates elements)
one compound → 2 or more elements and/or compounds AB → A + B 2H₂O → 2H₂ + O₂ AX → A + X
decomposition reaction
H₂ N₂ O₂ F₂ Cl₂ Br₂ I₂
diatomic elements
C₂Cl₆
dicarbon hexachloride
N₂S₃
dinitrogen trisulfide
Si₂Br₆
disilicon hexabromide
2 compounds → 2 different compounds AX + BY → AY + BX NaOH + HCl → NaCl + H₂O Pb(NO₃)₂ + 2KI → PbI₂ + 2KNO₃
double replacement reaction
Sigma bond
electrons are shared in an area centered between two atoms
Transition metal
element in groups 3-12 that is contained in the d-block of the periodic table and, with some exceptions, is characterized by a filled outermost s orbital of energy level n, and filled or partially filled d orbitals of energy
Metalloid
element that has physical and chemical properties of both metals and nonmetals
Representative elements
elements designed with an A; from groups 1, 2, and 13-18 in the modern periodic table, possessing a wide range of chemical and physical properties
noble gas
elements tend to react so that they acquire the electron structure of a ___
Cl, Se, Ar, etc
elements that are anions
Na, Mg, Li, etc
elements that are cations
Nonmetal
elements that are generally gases or dull, brittle solids that are poor conductors of heat and electricity
Ionization
energy to remove electrons (nobel gases highest)
double replacement reaction
exchange of (+) ions between 2 compounds and produces a precipitate, gas, or water
F₂ + 2KI → I₂ + 2KF
fluorine and potassium iodide
Oxidation number
for a monatomic ion, is equal to the change
hydro-
for binary acids, the hydrogen part of the compound is named using the prefix ___
Interstitial alloy
formed when the small holes in a metallic crystal are filled with smaller atoms (carbon steel)
Coordinate covalent bond
forms when one atom donates a pair of electrons to be shared with an atom or ion that needs two electrons to become stable (both electrons share)
Molecule
forms when two or more atoms covalently bond and is lower in potential energy than its constituent atoms
Empirical formula
formula that shows the smallest whole-number mole ratio of elements in a compound
Alkaline earth metal
group 2 elements in the modern periodic table and are highly reactive
Substitutional alloy
has atoms of the original metallic solid replaced by other metal atoms of similar size (sterling silver and 12 carat gold)
4 bonds
how many bonds does the carbon family have
1 bond
how many bonds does the halogen family have
3 bonds
how many bonds does the nitrogen family have
2 bonds
how many bonds does the oxygen family have
four
how many electrons are shared in a double covalent bond?
2 elements
how many elements does a binary elements?
1 (2,3,4,5,6,7)
how many valence electrons does group 1 have (group 2, 13,14,15,16,halogens?)
HBr
hydrobromic acid
HCl
hydrogen chloride
e⁻
if __ is under the arrow in an equation, it is electrolysis
one
if no number appears in the subscript place, the assumption is that the number equals ____
oxyanion
if such an ion is negatively charged and includes one or more oxygen atoms, it is called a ___
sigma bond
if the electrons shared are centered between the two atoms, the attachment is called a ___
-ic
if the name of the anion of an oxyacid ends in -ate, the acid name contains the suffix ___
pi bond
if the sharing involves the overlap of parallel orbitals, the attachment is called a ___
-ate
if two such ions can be formed that contain different numbers of oxygen atoms, the name for the ion with more oxygen atoms ends with the suffix ___
heat
if___ is over the arrow in an equation, reactants are heated
Combustion reaction
in a chemical, the number written in front of reactants with oxygen, releasing energy in the form of heat and light ex) the -> in a chemical equation
zero
in ionic compounds, the sum of the charges of all the ions equals to ___
terminal atom
in molecules, hydrogen is always a ___ (atom on the end)
mono-
in naming the first element in a formula, the prefix ___ is not used
cation; anion
in the chemical formula for any ionic compound, the chemical symbol for the ___ is written first, followed by the chemical symbol for the ___
Coefficient
in the chemical, the number written in front of a reactant or product, in the balanced equation describes the lowest whole number ratio of the amounts of all reactants and products ex) 2 in 2Fe(s)
32; 6(S) + 24(O) = 30 + 2 = 32
in the sulfate ion (SO₄²⁻), ___ electrons are available for bonding
as molecules containing two atoms
in what form do elements such as hydrogen, nitrogen, and oxygen normally occur?
Electronegativity
indicates the relative ability of an element's atoms to attract electrons in a chemical bond
Spectator ion
ion that does not participate in a reaction
polyatomic
ions made up of more than one atom are called ___ ions
negative
ions that have larger charges tend to produce a more ___ lattice energy than ions with smaller charges do
Fe(OH)₂
iron(II) hydroxide
FeBr₃
iron(III) bromide
less
large ions tend to produce a ___ negative value for lattice energy than smaller ions do
Pb₃(PO₄)₂
lead(II) phosphate
activity series
list of elements arranged according to the ease with which they undergo certain chemical reactions
LiF
lithium fluoride
Li₂S
lithium sulfide
MgBr₂ + Cl₂ → MgCl₂ + Br₂
magnesium bromide and chlorine
Mn₂O₇
manganese(VII) oxide
HgBr₂
mercury (II) bromide
salt 2KCl
metal + halogen →___ 2K + Cl₂ →___
metal oxide + carbon dioxide MgO + CO₂
metallic carbonate →____ +____ MgCO₃ → ___+___
metal chloride + oxygen 2NaCl + 3O₂
metallic chlorate → ___ + ___ 2NaClO₃ → ___+___
metal oxide + water CaO + H₂O
metallic hydroxide →___+___ Ca(OH)₂ →___+___
octet
most of these elements have a set of eight outermost electrons, which is called a stable ___
Salts
name for most ionic compounds other than oxides
gaining
nonmetals form a stable outer electron configuration by ___ electrons and becoming anions
combustion reaction
occurs when a substance reacts with oxygen, releasing energy in the form of heat and light
single-replacement reaction
one element replaces another element in a compound
Solute
one or more substances dissolved in a solution ex.) sugar/salt in water
Percent composition
percent of mass by each element in a compound
6K + Al₂O₃ → 2Al + 3K₂O
potassium and aluminum oxide
K₃PO₄
potssium phosphate
reactant type: single replacement
reactants: an element and a compound products: an element and a compound
reactant type: decomposition
reactants: one products: two or more
reactant type: combustion
reactants: one plus oxygen products: one or more oxides
reactant type: double replacement
reactants: two compounds products: two compounds
reactant type: synthesis
reactants: two or more products: one
Electron sea model
represents the way electrons exist in metals
valid lewis structure
resonance occurs when more than one ____ can be written for a molecule
(+)
separates 2 or more reactants/products
->
separates the reactants from products
AgCH₃COO
silver acetate
Ag₂O
silver oxide
decomposition reaction
single compound breaks down into 2 or more elements or compounds
A + BX → AX + B metal + compound → new compound and the replaced metal nonmetal + compound → new compound and the replaced nonmetal 2HCl + Zn → ZnCl₂ + H₂ Mg + 2HCl → H₂ + MgCl₂ MgBr₂ + Cl₂ → MgCl₂ + Br₂
single-replacement reaction
Na₂CO₃
sodium carbonate
Octet rule
states atoms lose, gain, or share electrons in order to acquire the stable electron configuration of a noble gas; 8; 8 electrons
Sr(NO₃)₂
strontium nitrate
lower right
subscripts are written to the __ of the symbol for the element
nucleus electrons ions
such an attachment may form by the attraction of the positively charged ____ of one atom for the negatively charged ___ of another atom, or by the attraction of charged atoms, which are called ____
SO
sulfur monoxide
H₂SO₃
sulfurous acid
A + B → AB 2Mg + O₂ → 2MgO 2H₂ + O₂ → 2H₂O
synthesis reaction
false; some of them are, some turn into long pairs
t/f all electrons in an atom are available for bonding
false; they are not
t/f the electrons in a coordinate covalent bond are donated by both the bonded atoms
TeCl₄
tellurium tetrachloride
noble gases
the ___ are a family of elements that have very little tendency to react
lattice energy
the ___ is the energy required to separate the ions of an ionic compound
crystal lattice
the ____ of ionic compounds affects their melting and boiling points
Metallic bond
the attraction of a metallic cation for delocalized electrons
valence energy level
the attractions may also involve ___ electrons, which are the electrons in the outermost ____
two
the carbon dioxide molecule contains ___ double bonds
lowest
the central atom in a molecule is the one with the ____ electron affinity
oxidation number electrons
the charge of such an ion is equal to the atom's ___, which is the number of ___ transferred to or from the atom to form the ion
Delocalized electron
the electrons involved in metallic bonding that are free to move easily from one atom to the next throughout the metal and are not attached to a particular atom
Ionic bond
the electrostatic force that holds oppositely charged particles together
lower
the energy of an ionic compound is ___ than that of the separate elements that formed it
Ionization energy
the energy required to remove an electron from an atom in its gaseous atom; generally increases in moving from left to right across a period and increases in moving down a group
Lattice energy
the energy required to separate one mole of the ions of an ionic compound, which is directly related to the size of the ions bonded and is also affected by the charge of the ions
Lanthanide series
the f-block elements from period 6 that follow the element lanthanum
Actinide series
the f-block elements from period 7 that follow the element actinium
chemical bond
the force that holds two atoms together is called a ____
Chemical bond
the force that holds two atoms together; may form by the attraction of a positive ion for a negative ion or by sharing electrons
reactant; reactant; product arrow, + sign, g, g, g
the fuel for the space shuttle is hydrogen, which burns in oxygen to produce water vapor and energy. in this chemical reaction, hydrogen is a __, oxygen is a ___, and water vapor is a __. in this chemical equation for this reaction, a ___ is used to separate hydrogen and oxygen from water vapor and energy. a ____ is used to separate the symbols for hydrogen and oxygen. a ___ symbol is used to tell the state of hydrogen in the reaction, a ___ symbol is used for the state of oxygen, and a ___ symbol is used for the state of water vapor
-ite
the name for the ion with fewer oxygen atoms ends with ___
number of electrons
the number of bonding pairs in a molecule is not equal to the ____
hexa-
the prefix ___ indicates six atoms
four
the prefix tetra- indicates __ atoms
Chemical reaction
the process by which the atoms of one or more substances are rearranged to form different substances *changes in temperature, color, odor, and physical state
pseudo-noble gas formations
the relatively stable electron structures developed by loss of electrons in certain elements of groups 3,4,13,14 are called ____
-ide
the second element in the formula of a binary compound is named using the suffix___
Solvent
the substance that dissolves a solute to form a solution; the most plentiful substance in the solution ex) water mixed with sugar/salt
negative
to find the total number of electrons available for bonding in a ___ ion, you should add the ion charge to the total number of valence electrons of the atoms present
law of conservation of mass
total mass of the reacting substances is always equal to the total mass of products
Skeleton equation
uses chemical formulas to identify reactants and products ex) 2 Fe(s) + 3Cl₂(g) -> 2FeCl₃(s)
Word equation
uses words to indicate reactants and products of chemical reactions ex) A + B -> AB Iron (s) + chlorine (g) -> Iron III chloride (s)
- adjust the coefficients to the smallest whole-number ratio (2,3,2) - coefficient appears in front of formula in a chemical equation - chemical equations are balanced when the same number of each kind of atom appears in the reactants and the products
what are the three steps in balancing equations?
can be either positive or negative
what charge are ions
positive
what charge is a nucleus
Oxygen
what is always present in a combustion reaction?
trigonal planar
what is the molecular shape of AlCl₃
linear
what is the molecular shape of BeCl₂
tetrahedral
what is the molecular shape of CH₄
trigonal pyramidal
what is the molecular shape of PH₃
octahedral
what is the molecular shape of SF₆
exothermic
when a covalent bond occurs, bond dissociation energy is released, and the process is ___
4
when carbon and oxygen bond, the molecule contains __ pairs of bonding electrons
covalent bond
when sharing of electrons occurs, the attachment between atoms that results is called a ___
molecule
when two or more atoms bond by means of electron sharing, the resulting particle is called a ___
the shorter the bond, the stronger the bond
which of the following relationships relating to bond length is generally correct?
2
write diatomic elements with ___ as the subscript
Zn(SCN)₂
zinc thiocyanate
