exam
what is an example of an ion formation
h+ is likely to lose one because it doesn't have a full shell
binary ionic
metal+ nonmetal
what are transition metals
Sc, Ti,V,Cr,Mn Fe co Ni Cu Zn
what do transition metals form
transition metals form cations by losing an electron
polyatomics
nitrate, sulfate, phosphate, biocarbonate, carbonate, hydroxide, acetate, chlorate, are the eight most common
what is the definition of acids
release h+ when dissolved in water occurs when positive charge is provided by h+
combining ions to make a formula units
Lead |V sulfide PB+4 S-2 (One pb4+ two s-2)
draw a Lewis structure for covalent
draw
what is the definition trends in IE
IE required to remove electron stronger attraction therefore more energy to remove an electron
what does the ie do
IE decrease, and size will increases
go across the PT, IE will increases size decreases
trend an IE explaining reactivity
Oakland Meadows become more reactive and decrease ionization energy well halogens have increased ionization energy and decreasing reactivity
what is the definition in trends in EA
they release or require to gain an electron therefore electron added can get to the nucleus = more attention
explain reactivity and trends in EA
halogens have high EA and are highly reactive, well noble gases have low EA which are unreactive
trends in EN by definition
the ability of an atom to attract shared electron, and share pair that can get to the nucleus therefore stronger traction
whats e n graph
0 to 0.5 is nonpolar covalent
0.5 to 1.7 is polar covalent
1.7 and up are ionic
explain why f is high
f has high e n because it's small size high effective nuclear charge therefore need to gain one electron to stable
definition of trend radius
size will decrease and increase at a decreasing rate it increases since electrons are added to a new shell usually the outer shell
what does radius do on the PT
across the periodic table size decreases like sodium due to their position on the PT is group one well c l is group 17 therefore Na is larger
how en explains why bonds are polar
EN(0.5-1.7) means the electrons are shared and that they sit close to EN Adam to make polar covalent bonds but for a larger like 1.7 and up indicates one atom attracts electrons much more than other atom gains possession (ions form)
indicating Bond polarity
the Chargers and Parker charges in molecule influence their properties bigger charge greater attraction
what are 3D structure predict molecule polarity
has polar bonds and draw
using classification of ionic versus polar versus nonpolar to explain MP and BP
the classification of substance as ionic polar and non-polar synthetically influenced melting points MP and boiling points BP
using classification of ionic versus polar versus nonpolar to explain solubility
Nonpolar molecules can't replace attraction don't dissolve in water
Ionic compounds would dissolve in water unless the compounds are strongly attracted
Polar molecules have partial charge attraction
what are characteristics of complete reactions
- Creates CO2 and H2O
-occurs sufficient o2 is presented
-produces blue flame and Max heat
what are characteristics of incomplete reaction
-create co poisonous gas and stoot and CO2 and HO2
-occurs when not enough o2 is presented
-produces yellow flame unless heat
combustion products characteristics
combustion refers to the raplid reaction with auction to reduce one or more oxides
predict products in double displacement reaction given in a soluble table
the positive ions of two ionic compounds exchange places example
producing a gas
producing water
producing a solid
predicting products in single displacement reaction given in an activity series
reactions to occur pure Meadow must be higher on the activity series example magnesium plus 2 hydrogen chloride produces magnesium chloride plus hydrogen
decomposition
one reactant becomes two or more products example h 2O2 produce o2 + H2O
synthesis
two or more reactants create one product
mg plus o2 produce two magnesium oxygen
single displacement
up here element reacts with an ion is solution
Cu + AgNo3 =Ag+ Cu No3)2
double displacement
two ionic compounds in a solution for a solid
(Ag No3+NaCl=AgCl+NaNo3
neutralization
acid plus base equals water
HCL+NaOH=H2O+NaCl
combustion
reaction with o2
what is a mole 6.02 * 10 ^ 23 things
represents the quantity of atoms molecules or particles in one mole
how many moles of source c12 h22o 11 contain total 2.8 * 10 ^ 25 atoms
molecule c12h22/11 = 2.88 * 10 ^ 25 atoms * 1 mole divided by 6.02 * 10 ^ 23 * 1 molecule divided by 45 mole equals 1.06 a molecules
what is the mass of 2.4 * 10 ^ 24 formula units of fe3 po4 2
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concepts of mole
converting molecules to formula units and moles
molecule/formula units to moles
moles equals number of molecules / 6.02 10 ^ 23
most molecule / formula units. if you have 0.500 moles of sodium chloride what is the formula
Fu=0.500 * 6.02 * 10 ^ 23 equals
converting number of ions / atoms to moles. you have one point 204 * 10 ^ 24 ions of sodium how many moles of NaCl does this
moles of NaCl=1.204 * 10 ^ 24 / 6.02 * 10 ^ 23
how many moles of H2O correspond to 3.612 * 10 ^ 24 hydrogen atoms
number molecules equals 3.612 * 10 ^ 24 / 2 moles of h2=
moles H2O=1.806 * 10 ^ 24 / 6.02 * 10 ^ 23
=
calculate molar mass for CH4
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how many moles is 100.0 mg (oh)2
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how many molecules is 5.0g CH4
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stoichiometry given moles of one compound find moles of another
right bounce equation
determine the mole ratio
and use more ratio calculate
example mole NH3 =moles h2.(5) x2/3 =
stoichiometry given mass and a balanced chemical equation find the mass of another compound
write a bounce equation
convert mass to moles (moles=Mass
molar mass)
limiting reaction-
limiting reaction is one that gets used first therefore limits the product to form reactant is left over is called ecses
given mass of two reactants find the mass of product
wtie a balanced equation
convert masses of reactants to moles
moles of reactant=mass of reactant
molar mass of reactant
limiting reaction question
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draw diagram to show aqueous solution for h 2co
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ionic and coval
ionic splits apart
covalent stays together
5 sources of errors
incomplete reaction
poor lab techniques resolving loss of reactant/product
competing reaction
product not dry
Impure reactants
what is the percent yo if 75.0 g of n2 reacts with h to make 17.2 g of NH3
calculate theoretical yield then calculate percentile
salute
other substance in a solution
soluent
substance that gives greater amount of solution
solution
homogeneous mixture two or more substance
aqueous solution
anything containing water
alloyed
is a solution of metals
saturated
solution that cannot dissolve solvent
unsaturated
solution that can dissolve solvent
supersaturated
contains more dissolved solvent than saturated solutions
miscible
forming homogeneous when added together
immiscible
incapable of mixing
soluble
a substance able to dissolve even in water
insoluble
incapable of dissolving
slightly soluble
solid substance dissolve in water between 0.1/10 g per liter
electronegativity
atom atract electrons that share Bond or take another atom to outershell
dipole
separation of charges within molecules between two bonded Adams or that share ionic bond
polar
water molecules enables water to dissolve wide range of solution
nonpolar
molecules that have no electrical charge or partial charge
dipole dipole
polar solute molecules is weaker than hydrogen
Hydrogen bonding
type of dipole dipole attraction between the molecules
ion dipole attraction
electrostatic force between ions and polar molecules
hydration
islands insoluble ionic compound to separate and disperse water one compounds dissolves
concentration
refers to the amount of salute in a given amount of solution
23.47 sample of road slush is dried and remaining salt weights 4.58 g what is the massal would be in 50.0 g of slush
percent Mass per Mass
what is percent volume if 10.00 ml ethanol is added to 20.0 ml water
volume per volume percent
what is the percent mass volume if 2.00 g of medication is dissolved to make 3.00 mL of solution
mass per volume percent
what is PPM and ppb used
is typically used in very diluted solutions
PPM =massive salute\mass of solution x10^6
molarity concentration
amount of salute / volume of solution
what is the morality of solution that contains 0.90 g of NaCl in 100.0 ml of solution
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dilution
dilution adding more solvent to solution therefore volume increase concentration decreases
when volume of 18 mol/l h2so4 is required to make 2.0 l of 0.10m/l h2so4
c1 v1 c2v2
stoichiometry involving solutions
one or more reactants in an aqueous solution
when aqueous solutions of beryllium chloride and sodium sulfate are mixed
bacl2+ na2so4=to NaCl+bas04 therefore is baso4 is insoluble
how pressure volume and temperature are related
pressure increases volume decreases until sufficient rate of collisions to equal external pressure
temperature increases pressure increases volume increases due to the particles moving faster when heated
particles don't attract or repel
cool down a gas enough theoretically particles stop moving therefore no space between them
temperature always will be 273° c
why the Kelvin temperature scale must be used
because it's an absolute temperature scale meaning that Ok is zero went through a clear molecular motion stops
ideal gas law
if you plot PV vs NT you get straight line
ideal gas law-what massive o2 gas would have a volume of 25 ml at 2.0 Atm and 15° c
mO2= v= T= P =