CHEM 120 Final Study Guide -Latest Update
CHEM 120 Final Study Guide
CHEM 120 Final Study Guide -Latest Update
Ionic Compounds
Are held together
... [Show More] by ionic bonds
Usually consist of a metal cation and a nonmetal anion
Always a metal and a nonmetal
Arranged in a crystal lattice
Each are more stable
Ex: lithium fluoride LiF 〖Li〗^+ and F^-
Covalent Bonding
Electrons are shared between atoms in pairs
Nonmetal and Nonmetal
Noble Gas electron configuration “8” valance electrons
Naming Ionic and Covalent bonds
Naming Ionic Compounds
Every chemical compound has its own specific name
State the name of the metal ion first then followed by the root name of the nonmetal with -ide ending
Ex: sodium oxide
Naming Covalent Compounds
Ex: carbon tetrachloride - 〖CCl〗_4
First start by naming the original elements
Carbon has 1 molecular while chlorine has 4
We add the pre-fix that means the number of molecules
Tetra- means 4
1 carbon and 4 chlorine
Add the suffix -ide to the end of the second element
Cu2SO4
Copper II sulfide
Whats The Bond
Combined gas law
Constant
R=0.08206
Volume has a direct affect with temperature
Atomic Number
The number of protons and electrons of an element
Isotopes
We will be given a number of protons and neutrons and have to determine which element it is by the number
Ex: 18 protons and 20 neutrons what is the isotope?
Argon
Poly Atomic Groups
Name
S^(2-) Sulfide Ion
〖SO〗_3^(2-) Sulfite Ion
〖SO〗_4^(2-) Sulfate Ion
〖NO〗_3^- Nitrate Ion
〖NO〗_2^- Nitrite Ion
N^(3-) Nitride Ion
〖PO〗_4^(3-) Phosphate Ion
P^(3-) Sulfide Ion
Balancing Equations
Combustion
Always produces H2O
2C4H10 + 1302 8CO2 +10H20
Neutralize
H2SO4 + 2KOH K2SO4 +2H2O
Produces K, S, NaCl and H2O
How to write a formula
K+ Cl-
Cancel out
KCl
Mols Per Liter
Molarity=mol/L
Find the Molarity
Moles per liter
Molarity=mol/L
6.25 grams (0.0250 mol) of CuSO4•5H2O is added to a 250-mL volumetric flask.
Water is added to the mark so that the total volume is 250.0 mL.
What is the molarity of this solution?
Molarity=(0.0250mol )/(0.250 L)=0.100 M
Molar Mass
Elements atomic mass but with g/mol on as the unit
Ex: NaCl 58.44 amu =58.44 g/mol
Mass/Volume Percent
Mass/ Volume percent = (grams of soulte)/(voulme of soultion) x100
Ex: The concentration of NaCl in a saline bag is 0.9%. Therefore, for every 100 mL of solution, the mass of NaCl present is 0.9 g.
0.9g/100mL x100=90%
Percent by Mass of Solute
Formula 𝑃𝑒𝑟𝑐𝑒𝑛𝑡 𝑀𝑎𝑠𝑠 𝑆𝑜𝑙𝑢𝑡𝑒=(𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒/𝑡𝑜𝑡𝑎𝑙 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛)𝑥100
What is the mass percent of NaCl in a solution that is prepared by adding 10.0 g NaCl to 50.0 g water?
Ex: 10.0𝑔/10.0𝑔+50.0𝑔𝑥100=16.7%
M1V1=M2V2
Volume vs. Amount of Gas
What types of nucleic acids do we have?
2 groups
DNA and RNA
What example of a polysaccharide?
Starch, glycogen and cellulose
What are amino acids?
Amino acids contain the –NH2 and –CO2H groups and a side chain.
Amine and Carboxyl
Difference between DNA and RNA
DNA
Double helix
A, G, C and T
RNA
Single helix
A, G, C and U
Replication•
Occurs in the nucleus
A process that copies DNA to make new DNA molecules during cell division
Assures new cell has same genetic information
Transcription•
Also occurs in the nucleus
A process of synthesizing various types of RNA using DNA as a template
Synthesized RNA is transported out of the cell nucleus to the cytoplasm
Translation
Occurs in the cytoplasm
A process using RNA to synthesize protein molecules from amino acids
Strands of DNA or RNA
Which protein or amino acid is formed?
Proteins are formed from 20 different amino acids
DNA is not directly involved in protein synthesis, but RNA is.
Lewis structure
Electron dot system
Each dot represents an electron
The element wants to be like the noble gas and have 8 valance electrons
D
D
D
Saturated
Single bond between carbon
Alkane
-ane
Formula C_n H_(2n-2)
Ex: CH3CH2CH2CH2
Unsaturated
Double or triple bonds between carbon
Double bond
Alkenes
-ene
Name
Alkenes are named with a prefix denoting the number of atoms in the longest chain followed by the ending –ene
Formula
CnH2n
Ex: H2C=CH-CH=CH2 is named 1,3-butadiene
Triple Bond
Alkynes
-nes
Naming
End with more than one of the same branch, use the prefixes di- or tri- to designate 2 or 3 of the same alkyl group.
Formula
CnH2n+1
EX: CH2CHCHCH
Polar
has a positive and negative side to the molecule
unequal sharing
Big difference in electronegativity then its polar covalent
Nonpolar
nonpolar bonds or has polar bonds arranged symmetrically.
Completely equal
No difference in electronegativity then its nonpolar covalent
Radiation
Danger Exposure
rem = roentgen equivalent for man
Single dose of 0-25 rem: no effect
25-100 rem: temporary blood cell changes
100-300 rem: radiation sickness; decrease in white blood cells
400-600 rem: 50% chance of death
>1000 rem: 100% chance of death
Normal exposure = 200 mrem (0.2 rem) per year, which produces no observable effects
Alpha Particles
Least harmful to humans
Loses 2 protons and 2 neutrons
Atomic number decreases by 2 and the mass number decreases by 4
Formula (_2^4)a
Ex (_90^232)Th-→(_88^228)Rh+(_2^4)a
Beta Particles
Can penetrate though skin into tissue
Atomic number increases by 1 and the mass number remains the same
Formula (_-1^0)B-
Ex:(_90^231)Th-→(_91^231)Pa+(_-1^0)B-
Gamma Rays
Most penetrating type of radiation
No change in mass or atomic number
Ex:〖(_^99m)Tc-→〗^ Tc+ y
Positron Emission
atomic number decreases by 1 and its mass number remains unchanged
Formula (_1^0)B+
Ex:(_12^23)Mg-→(_11^23)Na+(_1^0)B+
Electron Capture
mass number stays the same, but the atomic number decreases by 1
Formula (_-1^0)e-
Ex: (_4^7)Be+(_-1^0)e--→(_3^7)Li
Naming ochem’s
Meth-1
Eth-2
Pro-3
Bute-4
Pent-5
Hex-6
Hept-7
Oct-8
Non-9
Dec-10
Functional Groups
Alcohols
-OH
Ex: CH3OH
Ethers
-O-
Usually an oxygen between two carbons
Naming
CH3CH2-O-CH2CH3is named diethyl ether.
Aldehydes
R-CHO
C=O
Aldehydes always have an H attached
CH3CH2CHO
Ketones
C=O
Has C=O somewhere in the middle
(CH3)2CO
Carboxylic Acid
COOH
CH3CH2CO2H
Esters
RCO2R
CH3CO2CH2CH3
Amines
NH3
CH3CH2NH2
When using temperature always convert Celsius to Kalvin
K= 273.15
Oxidation-Reduction Reactions
Oxidation does not occur without reduction
Oxidation
The process of losing one or more electrons
Reduction
The process of gaining one or more electrons
Oxidizing Agent
A reactant that gains electrons and is reduced is the oxidizing agent because it accepts the electrons that are lost by the reactant that is oxidized
Reducing Agent
A reactant that loses electrons and is oxidized is the reducing agent because it provides electrons to the reactant that gets reduced.
Acid and Base
Acid
An acid donates an H+ ion to another substance
Base
A base accepts an H+ from another substance.
H2SO4(aq) + F–(aq) -> HSO4–(aq) + HF(aq)
H2SO4 is the acid
F- is the base
Reactions
In acid base reactions, the acid donates an H+ to a base.
Shapes
Strands of DNA or RNA
Which protein or ammio acid is formed?
What is the translated or transformation?
Find the molarity
Mols/mass [Show Less]