Chemistry Flashcards
Chemistry
study of matter (what matter is made of)
The things that make up stuff
the entities that comprise matter
Entities (biggest to smallest)
atoms (protons, electrons, neutrons), molecules, electrons
John Dalton
English schoolteacher- billiard ball (sphere) model
The Dalton Model
billiard ball/sphere- atom is indivisible
J.J Thomson
raisin bun model or plum pudding
Plum Pudding Model
electrons embedded into a positive fluid
Cathode ray tube
light cannot bend by itself it needs a charge (magnetic or electric)
- showed that the mass is 2000 times smaller than a hydrogen item
You can calculate what with strong magnets in a circle
charge and mass of particles
Ernest Rutherford
the gold foil experiment
The Gold Foil Experiment
expected the beam of particles to go right through the gold foil but instead some went different ways
Gold Foil Experiment proved that…
there was a small massive centre to the atom (nucleus) that caused them to deflect
Nuclear Model
Rutherford- small positive, densely packed nucleus (over 99% of the mass in the nucleus)
Planetary
Niels Bohr
Bohr Model found by the bright line spectra
Bohr Model
nucleus and electrons orbiting (excited state)
Excited State
add electricity and the electron jumps to the higher shell from the atom absorbing energy
Bright Line Spectra
when the electrons in the excited state drop back down a certain colour is emitted based on the energy level
Wave Mechanical Model
Erwin Schrodinger
Number of electrons in each shell
2, 8, 18, 32, 32, 18, 2
Bohr Model outer things
shells or orbits or energy levels
Wave Mechanical Model outer things
orbitals (Bohr orbits)
Periods
2 elements, 8, 8, 18, 18, 32, 32
18 groups
Alkali metals are
Extremely reactive- 1
Alkali metals
Li, Na, K, Rb, Cs
Alkali earth metals are
Quite reactive- 2
Alkali earth metals
Be, Mg, Ca, Sr, Ba, Ra
Transition metals
3-12
Halogens are
extremely reactive- 17
Halogens
F, Cl, Br, I
Noble gases are
stable- 18
Noble gases
He, Ne, Ar, Kr, Xe, Rn
An entity is stable when…
the valence shell is full
IUPAC
International Union of Pure and Applied Chemistry
Molecular
two non-metals
Common molecular compounds
Sucrose- C12H22O11(s), glucose- C6H12O6(s), water- H2O(l), ammonia- NH3(g), ozone- O3(g), methanol- CH3OH(l), ethanol- C2H5OH(l)
Naming molecular compounds
use the prefixes
Prefixes
- Mono-
- Di-
- Tri-
- Tetra-
- Penta-
- Hexa-
- Hepta-
- Octa-
- Ennea-
- Deca-
Ionic
one non-metal one metal (solids)
Types of Ionic Compounds
Binary, Multivalent, Polyatomic
Sucrose
C12H22O11 (s)
Glucose
C6H12O6 (s)
Ammonia
NH3 (g)
Ozone
O3 (g)
Methanol
CH3OH (l)
Ethanol
C2H5OH (l)
Binary (naming)
two elements
- MULTIPLY THE TWO CHARGES (LITTLE NUMBERS) TO MAKE THEM CANCEL EACH OTHER OUT
Multivalent (naming)
- MULTIPLY THE TWO CHARGES (LITTLE NUMBERS) TO MAKE THEM CANCEL EACH OTHER OUT AND THEN WHICH EVER OF THE TWO CHARGES YOU USED WILL BE THE ROMAN NUMERICAL
Polyatomic (naming)
- MULTIPLY THE TWO CHARGES (LITTLE NUMBERS) TO MAKE THEM CANCEL EACH OTHER OUT (using polyatomic ions)
Acids (5 indicators that can be seen)
- pH below 7 (lemon like 5 battery acid like 1)
- turns litmus paper red
- sour
- react with active metals (Mg, Zn, etc.)
- conduct electricity
Acid Indicator (cannot be seen)
- hydrogen (H)
- COOH will always be an acid
- all acids will be (aq)
Base (5 indicators that can be seen)
- pH above 7 (7 is neutral)
- turns litmus paper blue
- bitter
- feel slippery
- conduct electricity (electrolytes)
Base Indicator (cannot be seen)
- hydroxide (OH)
Aqueous means…
dissolved in water
Will mixing an acid and a base change the conductivity?
- no
- it will produce water and electrolytes
Every difference of one pH unit is an acidic difference of….
- 10
- ex. pH 8 to 4 is 10000 times more acidic
Isotopes
- Potassium is made of 19 protons and 19 neutrons
- some isotopes would have 21 neutrons some would have 20
- the .1 changes the amount
Atomic Number
- tells you how many PROTONS and ELECTRONS
Mass Number
- tells you the total number of protons and NEUTRONS added
Atomic mass minus atomic number…
- tells you the number of NEUTRONS
Why is water the universal solvent?
- it is a polar substance (O is negative and H and H are positive)
For acids ate goes to…
ide goes to….
- ic
- hydro _______ ic
If an ion is dissolved it is an ____________.
electrolyte
Element
cannot be broken down into any other substance (one atom)
Periods are
horizontal (7 of them)
Groups are
vertical (18 of them)
Do electrons farther away from the nucleus have more energy than those closer?
yes
Valence electrons
electrons in the OUTER energy level
Valence number
the number of electrons an element can gain or lose to combine with other elements
Ion
an atom where the number of electrons is not equal to the protons (has a net electric charge due to the loss or gain of electrons)
Precipitate
sometimes when ionic solutions are mixed they form a precipitate (a solid with low solubility that forms a solution)
When acids and bases are mixed… (neutralization)
when acids and bases react together both their acidic and basic properties disappear (process of neutralization)
Neutralization
acids and bases mixing and producing water and salt
Why do ionic solids have high melting points while molecular solids have low melting points?
- ionic solids have stronger attractive electrostatic (higher the attraction, higher melting point) (positive and negative attract strongly)
Electrolyte
a solution that conduct electricity (ionic compounds) (ions are able to flow and move)
Octect Rule
every atom wants to have 8 valance electrons in the outer most shell
Ionic Bonding
when elements bond to become stable (bonds between non-metals and metals)
Acid in Batteries
sulfuric acid
Acid in Vinegar
acitic acid
the most common multivalent is…
the top one on the chart
Electrons are the same number as
protons
Protons are the same number as
electrons
bottle of hydrochloric acid means what hazard symbol
corrosive
ionic are (conductor, melting point, solubility)
good conductor, high melting point, soluble
neutralize stomach acid with…
NaHCO3
photosynthesis formula
6CO2(g) + 6H2O —– 6O2(g) + C6H12O6 (exothermic)
law of conservation of mass
mass of reactants and products must be the same
reactants
left side of equation
products
right side of equation
endothermic
energy going in (takes in energy)
exothermic
energy going out (lets out energy)
cellular respiration formula
C6H12O6(aq) + 6O2 ——— 6CO2(g) + 6H2O(l) + energy
endothermic
anaerobic respiration
(bread, pizza dough)
- yeast is the enzyme (catalyst) digesting the sugar to produce gas to make the chemical reaction occur (not part of the reaction)
C6H12O6(s) ——-
2CO2(g) + 2C2H5OH(l)
airbags
energy + 2NaN3(s) ——- 2Na(s) + 3N2(g) (exothermic)
sodium azide
used in airbags NaN3(s) (decomposes into its elements)
Rusting
Fe(s) + O2(g) ——- Fe2O3(s)
BBQ
C3H8(g) + 5O2(g) ——– 3CO2(g) + 4H2O(g)
combustion of propane
diatomic
elements need (H2, Br2, etc.) in chart
ionic compounds are (s, l, g, aq)
solid
Acids are always (s, l, g, aq)
aqueous
Formation
a + b = ab
Decomposition
ab = a + b
combustion
CxHy + O2(g) = CO2 + H2O
single replacement
ab + c = ac + b or bc + a
double replacement
(displacement or neutralization) ab + cd + cb + ad
hydrogen w a match
pops
match ____ in CO2
goes out
match _____ in O2
gets bigger
Moles
used to count atoms, particles, molecules
Avogadro’s number (1 mol)
6.02 x 10 to the 23
1 mole is defined as
12g of pure carbon -12
n=m/M
chemical amount (mol) = mass (g) / molar mass (g/mol) - mass is is amount (g), chemical amount is moles, molar mass is in periodic table
how to find atoms or molecules
multiply the moles by 6.02 x 10 to the 23
How to read 2Na(s) + 2H2O(l) ——- H2(g) + 2NaOH(aq)
“2 moles of sodium react with 2 moles of water to produce 1 mole of hydrogen and 2 moles of sodium hydroxide”
How to find # of particles
n x N (moles times Avogadro’s number)
when writing equations do you put the positive or negative element first?
Positive
round to…
the same number of digits as the question gives you
