Section 1
Preview this deck
a reaction that releases energy
Front
| 5 | 0 | ||
| 4 | 0 | ||
| 3 | 0 | ||
| 2 | 0 | ||
| 1 | 0 |
Active users
2
All-time users
3
Favorites
0
Last updated
4 years ago
Date created
Mar 14, 2020
Cards (249)
Section 1
(50 cards)
a reaction that releases energy
exothermic reaction
This change you can see
physical change
Short hand electron configuration
putting the element that occupies the electron configuration shown except the last one which is written after it (e.g. potassium: (1s^2)(2s^2)(2p^6)(3s^2)(3p^6)(4s^1) and its short hand is [Ar] 4s^1)
If you can reverse the process through change-of-phase operations
physical change
energy required to get a chemical reaction started
Activation Energy
Massgravitational accelerationheight=mgh
Gravitational potential energy
quantum number that shows the angular momentum of the electron and the sublevel, which shows the orbital in which the electron could be within
ell
Properties that depend on the size of a sample
Extensive
Density is an extensive or intensive property
intensive
Property of metal that allows it to be hammered into thin sheets
Malleability
a force exerted over a distance
work
The total number of electrons a certain energy level can hold is
2n^2
Flammability, reactivity with acid, reactivity with oxygen, ability to decompose into specific elements
Chemical
a change that results in a new substance
chemical change
number of total protons and neutrons in an atom's nucleus
atomic number
Heterogeneous Substance
An unequal balance of different materials in a mixture
semimetals
semiconductors or metalloids which tend to be better conductors than non-metals but worse than metals
Change-of-phase operations
freezing, melting and evaporating
Properties that don't depend on the size of the sample
Intensive
atoms of the same element wit differing masses are called
isotopes
Properties that can only be observed by carrying out a chemical reaction
Chemical
the atomic mass unit (u) is based on an atom of what isotope
carbon-12
Homogeneous Substance
Possesses uniform composition
The normal boiling point of water
100 c
a substance made up of only one type of atom
monatomic element
quantum number used to indicate the energy level of an electron and it increases as it moves farther from the nucleus
n
ability to do work
energy
Electron configuration of oxygen
(1s^2)(2s^2)(2p^4)
have a definite shape and definite volume
solids
Properties that can be observed without carrying out a chemical reaction
Physical
quantum number that dictates the spatial orientation of the orbitals that the electron occupies
M sub ell or magnetic quantum number
An elemental form as two-atom molecule
diatomic
True solids possess what type of structure
crystalline
Electron configuration of hydrogen
1s^1
Electron Configuration
(energy level)(sublevel letter)^(number of electrons in sublevel)
When a substance is aqueous it is what type of mixture
homogeneous mixture
If you cannot reverse the process through change-of-phase operations
chemical change
quantum number that shows the spin direction of an electron in a certain orbital and differentiates the states of two electrons in the same orbital
M sub s or spin quantum number
A compound composed of three elements
A ternary compund
the process by which a solid turns directly to a gas
sublimation
This change you cant see
chemical change
the process by which a solid turns to a liquid
Fusion or melting
Mass, volume and weight are extensive or intensive properties
extensive
the process by which a gas turns directly to a solid
Deposition
Color, texture, density, freezing point, electrical conductivity, luster, hardness, mass and weight are physical or chemical properties
Physical
the process by which a liquid becomes a solid
solidification or freezing
a substance that is dissolved in water
aqueous
a reaction that results in a product at a higher energy level than the initial reactants
Endothermic reaction
energy of matter in motion
kinetic energy
Substance that is physically combined
Mixture
Section 2
(50 cards)
organic compound with carbon connected by multiple types of bonds
Unsaturated compounds
A molecule with a positive and negative side
polar molecule
poor conductors in any state, but good insulators of heat and electricity
Molecular compounds
What formula can be used to calculate the number of hydrogen atoms in a hydrocarbon, where n=# of carbon atoms
C(n)H(2n)=2n(n)
Have high melting and freezing points
Ionic compounds
If hydrocarbon is saturated it is given what suffix
-ane
If Na4 was given what would you NOT do to find its electronegativity
You would not multiply the electronegativity of Na by four, you will use just the normal form
Bond with similar compounds to make a bigger whole
Molecular compounds
This diagram of showing bonds uses lines to show covalent bonds. The number of lines are the number of bonds between the two atoms (or the shared electrons divided by two)
Structural formula
The forces that keep compounds together
Intermolecular forces
A molecule without negative or positive sides
non-polar molecule
These compounds don't bond with compounds of the same makeup, instead they crystalize
Ionic compounds, like table salt that have separate grains of crystallized ionic compounds
horizontal rows of the periodic table
periods
organic compounds with carbon connected by single bonds only
Saturated compounds
What type of bond has an electronegative difference of 0.4-1.7
polar covalent bond
Compound with only carbon and hydrogen
hydrocarbon
Hydrocarbon with only one carbon atom has what prefix
meth-
Analogy: What type of compound is like a crowd of families or couples where each person has a special relationship with another
Molecular compound
Positive ion
Cation
Bond with compounds of the same makeup and create a larger whole with all the same compounds (covalent)
Molecular compounds (e.g. H2O)
a bond formed when atoms share one or more pairs of electrons relatively equally
Non-polar covalent bond
When a four atom compound's main element gets bonded left and right and then on the bottom (e.g. BH3)
Trigonal planar
If Oxygen (O) gained two electrons what would it become
O(2-) because it only gained electrons not protons so it stays the same element but becomes an ion
Saturated hydrocarbons are in what group
alkane
What type of bond has an electronegative difference of greater than 1.7
Ionic bond
What type of bond has an electronegative difference of 0-0.3
non-polar covalent bond
Negative ion
Anion
Must have polar covalent bonds and must be asymmetrical
polar molecule
Two or more compounds that have the same molecular formula but different structural formulas
Isomers
If the molecule is geometrically symmetrical
non-polar molecule
When a compound contains both ionic and covalent bonds
Polyatomic ions - ions made up of more than one atom so multiple bonds can form between different atoms
When a three atom compound's main element can not share all of its electrons, thus causing an extra repulsive force
bent (Bonding should appear bent when shown on Lewis Dot Diagrams)
When a three atom compound's main element (e.g. CO2 main element is C) can share all of its electrons
Linear (the bonding should appear to be in a line when shown on Lewis Dot Diagrams)
columns of the periodic table
groups of families
An elements relative measure of its attraction for bonding electrons
electronegativity
elements in the first column of the periodic table
alkali metals
Analogy: What type of compound is like a crowd of strangers who have no relation to one another
Ionic compound
When atoms share electrons to fill their valance shell
Covalent bond(e.g. N2+O2 -> 2NO or 2H2+O2 -> 2HO2)
If hydrocarbon is double bonded it is given what suffix
-ene
a bond formed when atoms share one or more pairs of electrons but one atom attracts the electrons more strongly, resulting in unequal sharing
Polar covalent bond
The formation of a diatomic compound's nuclie
linear
When anions bond with cations to create a neutral charged compound
Ionic compound(e.g. Ca(2+) + O(2-) -> CaO)
A covalent bond where a shared pair of electrons between two atoms in only provided by one of them
Coordinate covalent bond
Ionic compounds are called what?
Salts
Most electromagnetic element
flourine (4.0)
Na and Cl make up table salt. What is each grain made of and what are they?
Each grain is made of the ionic compound of NaCl, with each also being a crystal. This makes the table salt an ionic crystal
Usually don't conduct electricity in the solid state, but they are good conductors in molten or a aqueous(solution) form
Ionic compounds
compounds containing carbon
organic compounds
If hydrocarbon has one or more triple bonds it is given what suffix
-yne
Prefix given to hydrocarbons with three carbon atoms
prop-
Section 3
(50 cards)
What is the oxidation number of Al
3+
Molecular formulas
Keep all the subscripts and gives all the information
What type of reaction is this: CH(4)+2O(2) -> CO(2)+2H(2)O
Combustion Reaction
What are the substances on the left-hand side of the arrow in a chemical equation
Reactants
How are binary compounds named
The more electronegative element goes first and is followed by the other element with a profix ide
When mass is converted into energy so elements can turns into other elements
Nuclear equations
What type of reaction is this: K+NaCl -> KCl+Na
Single replacement with metal
When an element and a compound react together and one element in the compound leaves to join with the previously alone element (Metals(A is the metal): A+BC->AC+B this is because A will only attract the element B or C depending on whether it has an opposite oxidation sign, so if it is -1 it will only take the element in the compound that had a positive number) (Non-metals: A+BC->AB+C this is different because A is no longer a metal so it will attract a different element)
Single Replacement
A polyatomic ion usually has what profix
-ate
Formula unit
The mass for the simplest ratio of cations to anions (e.g. NaCl the formula unit would be Na(+1) to Cl(-1))
Do not have any bonds, and have an oxidation number of 0
free element
How would you find the molecular formula given the empirical formula and the molecular formula's molecular mass
1) Find the mass of the given empirical formula 2) Divide the molecular mass by the empirical mass 3) Multiply the empirical subscripts by the given quotient
If an element is reduced what does it mean
the oxidation number has gone down due to gain in electrons
When two ionic compounds react in an aqueous solution, and an ion from one compound replaces the similar ion from the other compound (AB+CD -> CB+AD)
Double replacement
When a more complex substance breaks down into two or more simpler substances, that could be elements or compounds (AB -> A+B)
Decomposition reaction
What is the equation to convert between empirical or molecular
x= (Molecular mass)/(Empirical mass) To get molecular formula: CxH2xOx=C6H12O6 To get empirical formula: C6/xH12/xO6/x=CH2O
When two or more simple compounds or elements combine to form a more complex substance (A+B -> AB)
Synthesis reaction
Molecular mass
The mass of molecular compounds ONLY
How to find the mass of any compound
Look at all the elements in the compound and find their masses on the periodic table, then use these masses and add them up based on how many times that element appears in the compound.
(1)0^e
positron
(-1)0^e
Beta particle
The element or compound that causes the loss of electrons in another element (Element takes electrons)
oxidizing agent
What reaction is this: 2H(2)+O(2)->2H(2)O
Synthesis reaction
Formula mass
The mass of one formula unit
What are the five categories of chemical reactions
Synthesis, Decomposition, Single replacement, Double replacement, and Combustion
What type of reaction is this: Ba(OH)(2)+H(2)SO(4) -> BaSO(4)+2H(2)O
Double replacement
Can the subscripts in a chemical equation ever be changed while balancing?
No, only the coefficients
If there is a polyatomic ion what cannot be changed
The subscript or in other words the amount of it (You can multiply it like this: (NO3)2
What happens if the molecular formula cannot be reduced
Both the molecular and empirical formulas will be the same
How to find the oxidation number of an element?
Find how many electrons it would have to gain or loose to to fill its valence shell and which ever contains the least is the number
Mnemonic device for the five major categories of chemical reactions
Sally Dyed Sammy's red Dog really Crudely
What is an element called when it looses electrons after a reaction (e.g. C+O(2) -> C^4+O(2)^2-)
oxidized (Carbon in the example)
What is an element called when is gains electrons after a reaction (e.g. C+O(2) -> C^4+O(2)^2-)
reduction (Oxygen in the example)
(1)1^p
proton
How to find the correct chemical formula for a compound
Take the oxidation of all the elements and add more ions using subscripts in order to make it neutral
How to find the empirical formula with the percent composition of mass of a compound
1) Assume your dealing with a 100-gram sample (e.g. 28.5% Oxygen and 71.5% Calcium = 28.5 grams of Oxygen an 71.5 grams of Calcium) 2)Divide these masses by their masses from the periodic table (e.g. Calcium -> 71.5/40.1=1.78 parts Oxygen -> 28.5/16=1.78 parts) 3) find the ratio of these two quotients (e.g. 1.78:1.78=1:1) 4) Use this ratio to get the empirical formula (e.g. CaO)
What is hydrogen's oxidation number in a hydride compound
-1
(2)4^He
Alpha particle
A superscript showing the oxidation number of a polyatomic ion is different than when it is present on singe ions
It applies to the entire polyatomic ion, and isn't multiplied by the subscript
How are binary compounds written if an element can have multiple oxidation numbers but only one fits the current compound
With the needed oxidation number written in roman numerals in parenthesis after the element in question
(19)40^K (Not real notation look in book pg.78)
19 = nuclear charge 40 = mass number
What reaction is this: CaCO(3)->CaO+CO(2)
Decomposition reaction
What is the difference between a coefficient and subscript in a formula
A subscript shows connected elements or compounds while a coefficient shows individual elements or compounds (e.g. C6H12O6 would show all these atoms are together and work as a whole, while 6CO2 shows 6 CO2 pieces that are in the formula)
The element that causes the gain of electrons in another element (element gives electrons)
Reducing agent
When a hydrocarbon reacts with oxygen to produce water and carbon dioxide (Hydrocarbon+Oxygen -> Carbon Dioxide+Water)
Combustion Reaction
Equations that show the individual ions that exist in a solution
Ionic equation
What are the substances on the right-hand side of the arrow in a chemical equation
Products
What compounds are measured with formula mass
Ionic compounds
Empirical formulas
When all the subscripts are simplified (divided) e.g. C6H12 = CH6
(0)1^n
neutron
Section 4
(50 cards)
What law states: The volume of a gas decreases as the temperature(ONLY KELVIN) decreases and vise versa
Charles's Law
Solvent
substance that does the dissolving
Solubility
the ability of a substance to dissolve in another substance
Formula for Charles's Law (ONLY KELVIN)
V(1)/T(1)=V(2)/T(2)
Supersaturated Solution
When a large quantity of solute is applied relative to the ratio of grams of solute to solvent
Examples of units that measure pressure
Pascals, atm, torr, mm or mercury (mm of Hg)
Equation for Boyle's Law
P(1)V(1)=P(2)V(2)
In the IGL V=?
Volume
In the IGL n=?
Number of moles
Why are Ideal Gases a thing
All gases are treated like ideal gases in order to do calculations
Combined Gas Law Equation
V(2)=[V(1)P(1)T(2)]/[P(2)T(1)]
What does Avogadro's Principle tell us?
equal volumes of gases, at equal temperatures and pressures, contain an equal number of particles
Dry gas
A gas not including water
Atomic mass
Mass of one atom of that element
What are the two points stated by the KMT(Kinetic Molecular Theory)
- all gases are made of individual particles - the net kinetic energy of a gas stays the same despite particle collisions
Conversions of above units
1 atm = 101.3 kPa = 760 torr = 760 mm of Hg 1 kPa = 7.5 mm of Hg
Mole to Mole ratios
In a chemical equation you can look at the coefficients to get the mole ratios (e.g. 2C4H2+O2 the mole ratio would be 2:1 and for every 2 moles of C4H2 molecules there will be 1 mole of O2)
In the IGL P=?
Pressure
How is atmospheric pressure measured
with a devise called a barometer or closed manometer
One mole of STP gas will occupy what volume
22.4 dm^3
What if an element is in excess
it will never run out so you don't have to incorporate it during solving problems with them
Equation for Graham's Law
V(1)/V(2) = sqrt(M(1)/M(2))
Saturated Solution
When too much solute is present in the solution based on the temperature so it doesn't all dissolve (e.g. chocolate at bottom after drinking hot chocolate)
Ideal Gas Law
Show the relationship between pressure, volume, temperature, and number of particles of a gas
Graham's Law
The speed of gases based on pressure and temperature
In the IGL R=?
Ideal Gas Constant=8.31
STP
Standard Temperature and Pressure
Formula for Dalton's Law
P(total) = P(1)+P(2)+P(3)......
Solute
substance that gets dissolved into a solution
Limiting Reactant
The substance on the reactant side of a formula that will get used up by the reaction
Immiscible
When two liquids fail to mix
Volume of gas (STP) -> Moles of gas (STP)
volume of gas (STP)/22.4=moles
How much MgO is produced by 2g of Mg reacting with an excess of O ( 2MgO+O2->2MgO)
2Mg = 2/24.3 = 0.0823 moles ratio 2:2 = 1:1 so the 2MgO produced = 0.0823*40.3=3.32 g
What law states: if you change the volume of a gas, without changing temperature or number of particles of the gas, you get an inversely proportional change in the gas sample's pressure.
Boyle's Law
What law states: the total pressure exerted by a mixture of gases is equal to the sum of each of the partial pressures(pressure of each individual gas) of the gases in the mixture
Dalton's Law
Unsaturated Solution
When a solution is holding less solute than it can at that temperature, because when solutes are in a solvent a certain ratio in grams in present based on the temperature
Formula for pressure
Pressure = Force/Area
In all nuclear equation what two values must be conserved
The nuclear charge and mass number
How to calculate the pressure of a dry gas by removing that of the water vapor's pressure
1) Measure the temperature of the sample 2) Look at a Vapor Pressure of Water chart to find the pressure of the water vapor based on the temperature 3) Subtract that pressure of the total pressure
Ideal Gas Law Equation
PV=nRT
How to find the molar mass of an element
Take the atomic mass and instead of atomic mass units use grams (e.g. Carbon = 12 u so the molar mass of carbon is 12 g)
Molarity
A measurement for the concentration of a solution
Miscible
When liquids mix well
In the IGL T=?
Temperature (Kelvin)
Standard Temperature
273 K->31.73 Fahrenheit -> -0.15 Celsius
Properties of Ideal Gases
1) The molecules in the gas take up no space (most gases have molecules that take up very little space) 2) No attraction between particles in gas
Molar mass
the mass of 6.02*10^23 pieces
What is a Mole (Avogadro's number)
6.02*10^23 and it is a quantity like a dozen describes 12 things
Standard Pressure
101.3 kPa
Mole arithmetic
Mass -> Mole: Total Mass/mass in one mole=moles Moles->Mass: Moles * mass in one mole = mass Moles->Particles: (6.0210^23) moles = particles
Section 5
(49 cards)