Functional Groups

Let's get down to business. Today in class, we learned about functional groups. These are groups of atoms that exist in a molecule, and can give it special properties.

ALCOHOL is an organic compound that contains an OH group. The OH group is a functional group. When a hydrocarbon chain has an OH group, the name of the parent hydrocarbon changes. For example, pentane would become pentanol. 


This is methanol: CH3-OH

This is ethanol: CH3-CH2-OH 

This is 2-butanol: CH3-CH-CH2-CH3
                                  I
                                OH

This is 5-methyl-3-hexanol: CH3-CH2-CH-CH2-CH-CH3
                                                         I            I
                                                        CH3      OH


When you name an alcohol, name it so that the OH gets the lowest number possible. So if there is an OH group attached to the end of pentanol (5 carbons), name it 1-pentanol instead of 5-pentanol. (1 is lower than 5)

An ALDEHYDE is an organic compound that contains a C=O group at the end of a hydrocarbon chain- it can also be written as -CHO. These are named with "-al" at the end of the parent hydrocarbon. For example, hexane would be called hexanal. 


This is methanal: O
                            II
                       H-C-H


This is ethanal: CH3-CHO 
                         or
                         CH3-CH
                                   II
                                   O


KETONES are organic compounds that contain a C=O group at a position that's NOT at the end of a hydrocarbon chain. These are named with the ending "-one". 


This is propanone: CH3-C-CH3
                                       II
                                       O

OR

                                CH3COCH3 (condensed structure)

This is hexanone: CH3CH2COCH2CH2CH3

OR

CH3-CH2-C-CH2-CH2-CH3
                  II
                  O

ORGANIC CHEMISTRY GETTING EVEN MORE FIESTY.

Hi all,
as you may recall, last blog we talked about the wonderful world of alkanes. But it was a little plain, no? Now you have the chance to spice it up a little bit with adding in a few doubles bonds here, and a few triple bonds there. Let's start off with a few definitions:
Alkene: An organic compound containing a double bond between two carbons.
Alkyne: An organic compound containing a triple bond between two carbons.
Now we've established the difference between those two, we can get down to business.

 This is an alkene. Note the double bond.

How to name alkenes? You would name it just like alkanes, except changing the -ane to a -ene. For example, in the above image, there are two carbons. If you were writing an alkane, it would be ETHANE. However, because of the double bond, it is an alkene. Thus, the name for the above compound would be ETHENE.

Drawing them is a different matter. "How would we know where the double bond goes?", you may ask. Here is a better example to work with than the above:

 Meet hexene. As you can see, his double bond is in the middle of the schmongle. Recall how to write alkanes. Note that the carbon with the double bond is the 3rd one from the left/right. So we wouldn't have to bother with worrying about the smallest number. Since the double bond is on the 3rd carbon, we would name this 3-hexene. So drawing them would be the same matter. Just the corresponding number to where the double or triple bond is.

 Now meet ethyne. Ethyne is an alkyne. How do we know? See that triple bond there basking in it's glory? That's how we know.

Dealing with alkynes may look exhausting because of the triple bond, but do not fear. You'd be glad to hear that you do exactly what you've been doing all along with alkanes and alkenes. Just always, ALWAYS, remember to label where the triple bond is.

TMFAQ (The Most Frequently Asked Question)

Promising title isn't it? But the question is: What if we have a branch AND a double/triple bond?! What do I do with the naming? Would the branch be a priority for the "lowest number" used in describing the compound or would I use the location of the double/triple bond and then do things accordingly?! SAY WHAT?

Calm down, my young disciples. If something looked like this: 

You will ALWAYS, prioritize the double bond first. Same with triple bonds (alkynes). THEN, you do things accordingly. Therefore, this would be 2-methyl-3-hexene. 

YA DIG?

 Calvin's take on "OChem"...

Organic Chemistry!!! Chemistry that is healthy for you.

Today we are going to learn about ORGANIC CHEMISTRY. Excited? I think so.


Let's review exactly what organic chemistry is:

• The chemistry of carbon compounds
• Responsible for many everyday products like: your clothing, plastic, and alcohol

Properties

• Low melting points
• Weak or No-electrolytes

Types of Carbon Atom Chains

• A straight-line 
•   a circular pattern
•  a branched pattern

Types of Links with Other Atoms

 single bonds

 double bonds

 triple bonds

Moving on, a hydrocarbon is a compound containing only hydrogen and carbon.

Hydrocarbons come in different types and can be represented in different ways. 

Alkanes are saturated hydrocarbon where carbon atoms are bonded by single bonds.

(saturated: atoms cannot bond to the structure)

When naming Alkanes: The names of all hydrocarbons end in "ane"

This is a table of the main alkanes and their chemical formulas:

This table above is a homologous series.

Homologous Series: A series of organic compounds with similar general formulas and chemical properties

THE GENERAL FORMULA OF AN ALKANE

Some hydrocarbons are called substituted hydrocarbons or branched hydrocarbons because they are attached to the side of the original hydrocarbon

Now let's move on to Alkyl Groups.

An Alkyl Group is an alkane which lost one hydrogen atom

The names of all alkyl groups end in '-yl'

For example: Propane -> Propyl

With more of the same kind of alkyl group, the prefixes "di, tri, tetra, etc" come in to play

List the different groups alphabetically, ex/ Ethyl is before Methyl

Put the position number in front, and a dash between each alkyl group and it's number

To better understand the naming of Alkyl Groups, click this link:

New Chemical Bonds that will Blow Your Mind!!!!

Recently in Ms. Chen's class, we have learned new types of chemical bonds that I have never dealt with before! They are:

1. Non Polar Covalent Bonds: if electrons are shared equally
2. Covalent Bonds: if electrons are shared unequally
3. Ionic Bonds: if the electrons are transferred between 2 atoms

Before I get into explaining, let's review the basics of Electrostatic Force:

Electrostatic Force is a force that exists between charged particles as a result of attraction/repulsion. This operates equally in all directions.

• Opposite charges attract
• Like charges repel
• The greater the distance between two charged particles, the smaller the attractive force
• The greater charge on the particles, the greater the force of attraction

Typically, atoms with higher electro negativity strongly attract electrons from neighboring atoms. 

The trends for Electronegativity are the same as the trends for Ionization.

This is because, metals have low electronegativity and non metals have high electronegativity resulting in high ionization energies

You can measure electronegativity using the "Pauling Scale"

Electronegativity Difference = [Energy1 - Energy2]

1) IF ENeg Diff. < 0.5 it is a COVALENT BOND

2) IF ENeg Diff. > 0.5 and < 1.8 it is a POLAR COVALENT BOND

3) IF ENeg Diff. > 1.8 it is an IONIC BOND

NOW we will move on to intermolecular forces. These hold together individual molecules containing intramolecular covalent bonds forming covalent compounds.

How to differentiate between the two?

INTRAmolecular forces are found within a molecule, responsible for holding the atoms of a molecule together

INTERmolecular forces are found between the molecules, responsible for the bonding between molecules

Now you may ask, why do some bonds have low melting points? Well the answer to that question is simply because of weak bonds

                - During the melting process, only the weak bonds are affected. The covalent bonds 

                  within each individual molecule are not broken.

The LONDON FORCES are the weakest intermolecular force. This is due to temporary dipolar attractions between neighbouring atoms

A dipole is a partial separation of charge, existing when one end of a molecule has a slight positive charge and the other end has a slight negative charge

POLARITY

 > Outlines a molecule's electrical balance

 > If there is an imbalance with electrical charge, then the molecule is polar, if it is balanced, it is 

    non polar

Atoms with Higher Electronegativity will form a PARTIAL NEGATIVE charge

δ- (between 0 and -1)

Atoms with Lower Electronegativity will form a PARTIAL POSITIVE charge

δ+(between 0 and +1)

Example: NH3

N: 3.04

H: 2.20

3.04-2.20 = 0.84 meaning it is a polar covalent bond

Here are videos to sum up everything in this blog: 

Taking Representing Compounds in Diagrams to a Whole. New. Level. ELECTRON DOT AND LEWIS DIAGRAMS

Helloooo readers.


It is now time to take the next step in your relationship with compounds and represent them in what is called "Electron Dot and Lewis" Diagrams. YESS!! -insert confetti-


Now you must be asking how would you ever represent them in that way? Well I will start off by explaining exactly what a Lewis Diagram is.


A Lewis Dot Diagram is a diagram that shows the bonding between atoms of a molecule and the lone valence pairs in the molecule.

• The symbol of the element is in the center, and electrons are represented by dots surrounding it
• In total, there are 4 orbitals surrounding the element, each holding a maximum of 2 electrons
• 8 electrons represents a "closed shell" or "noble gas" configuration

Example Time!!!

Let's show the Lewis Diagram of Chlorine. 

Chlorine has 7 valence electrons, therefore in the Lewis Diagram, there are 3 full orbitals and 1 half full orbital

These are the Lewis Diagrams for part of the Periodic Table

Now let's do an example of a Lewis Dot Diagram for a compound

NF3

-In order to complete it's outer shell to make it contain 8 valence electrons, atoms gain, lose, or share electrons

-Carbon, Nitrogen, Oxygen, and Fluorine always follow this rule

• In this case, Nitrogen needed 3 electrons, and fluorine only needs 1 electron, therefore, nitrogen shares 3 bonds with 3 fluorines

Now, this is the Structural form of NF3

AWESOME GUYS. : D

This is a video to help you further understand the Lewis Dot Diagrams:

Periodic Table Trends

There are many trends that can be identified on the periodic table of elements. The ones that we will be reviewing today include:

• Metallic Properties
• Atomic Radius
• Ionization Energy
• Electronegativity
• Reactivity
• Ion Charge
• Melting/Boiling Point
• Density

Density: Elements become more dense as we reach the middle of the periodic table.

Metallic Properties: Elements go from metallic -> non-metallic as we go from left to right on the periodic table. Elements at the bottom of a group are more metallic than those at the top of the group. 

Melting/Boiling Point: Elements at towards the centre of the table have the highest boiling points. Noble gases have the lowest melting point. 

Ionization Energy: This is the energy required to remove one electron from a neutral atom. This trend increases upwards towards to right of the periodic table. Meaning that helium has the highest ionization (holding tightly onto its electrons because it has a perfect full shell) energy, and francium has the lowest (eager to get rid of its one valence electron). Ionization energy is given in kj/mol.  

Electronegativity: This is basically a way of saying how much an atom wants to gain electrons. Noble gases are excluded from this trend because they already have a full valence shell, and therefore do not need to gain or lose any electrons. 

The trend of electronegativity is basically the same as ionization energy. So it goes up and to the right. Fluorine is the most electronegative element. 

High electronegativity: This atom strongly attracts neighbouring electrons, and may quite possibly even remove it. At the same time this atom holds tightly onto its own electrons. 

Low electronegativity: This element doesn't attract neighbouring electrons very well, in fact, it even allows its own electrons to be easily removed. 

Atomic Radius: The atomic radius decreases as we move towards to right side of the periodic table. Reason being that there are more protons and electrons, causing more attraction, which packs the atom together more tightly. The atomic radius increases down a group, because as you go downwards, the elements atoms have more shells which make the atom larger. 

Reactivity: Atoms that are closer to getting a full valence shell (by either gaining or losing electrons) tend to be more reactive. Noble gases are very stable because they already have a full shell. 

LET'S GET UP-CLOSE AND PERSONAL WITH THE PERIODIC TABLE

So. I know you all have established some sort of relationship with your periodic tables now. I mean, come on, you use it to find out what the symbol for each element is, atomic numbers, ion charges, and atomic masses. Don't tell me you haven't fallen in love with the handy dandy bundle of joy and data. While all that is very appealing to our academic senses, haven't you ever thought of knowing about it a little more deeply? Haven't you ever wondered where all the information came from? And how families got grouped together? (Yes, that was my attempt on a pun). Afterall, like Bruce Lee says "Knowing is not enough; we must apply. Willing is not enough; we must do". How are we supposed to apply all this data if we don't know enough about the Periodic Table? Insightful, no?

In the beginning, scientists knew there were elements that acted out on certain things. But of course the number of those elements were limited. It all started with Aristotle's theory, saying that there were "elements": Fire, Earth, Water, Air. But by 1817, 52 elements were discovered, and scientists were already starting to organize them, or more so, "group" them. In 1857, a good man named William Odling organized the found elements of that time into 13 groups based on their similarities in physical and chemical properties.

The 19th Century was a breakthrough for the Periodic Table. The Law of Octaves was created by John Newlands, stating that chemical elements are arranged according to their atomic weight. He was one of the first scientists who detected a trend or pattern in the elements discovered. This was quite the breakthrough, however Newland's method didn't let scientist predict elements, and he made things ambiguous; he couldn't make his mind up and kept on changing the way he ordered things. Sounds like a confused, smart guy, eh?

Now, Newland must've been so aggravated when Mendeleev discovered something even more greater than he did. It was one of those "I knew that!" moments for him. Dimitri Mendeleev discovered that when you listed the elements in order according to their mass, certain features of elements recurred. Thus, he decided to organize the elements in periods (rows) and groups/families (columns). He even was smart enough to leave gaps in between elements for elements that would be discovered later on. This allowed scientists to predict elements according to their family and their similar properties.

In modern day chemistry society, (aka now), the elements are arranged according to their atomic number as opposed to their atomic mass.

But seriously, you students. Imagine if none of these scientist never made any of these discoveries. We wouldn't be sitting here doing chemistry. Dang. LOL jk.

.....Well that's one way to look at it.

Electron Configuration

Electron configuration is a method of describing the orbitals in which electrons occupy, it also states the number of electrons in each orbital. (maximum is 2)

Just to show you what it looks like, here is the electron configuration for silicon:

1s² 2s² 2p⁶ 3s² 3p² 

You see, electrons only exist in certain energy states. When the electrons absorb or emit a specific amount of energy, it will instantly jump to another orbital. The energy level is basically that amount that an electron of an atom can have. This is called "n". 

The energy difference between 2 energy levels is called the quantum of energy.

Atoms can exist in 2 states:

Ground State: all electrons of the atom are at their lowest possible energy level

Excited State: one or more electron is in an energy level other than the lowest possible one

Here are some other things that you should know:

Orbital: the actual amount of space that is being occupied by an electron

Shell: the set of all orbitals that have the name n-value

Subshell: a set of orbitals of the same type (like 2s and 2p)

s, p, d, and f refer to four types of orbitals.

An atom's electron shells are filled according to the following theoretical constraints:

• Each s subshell holds at most 2 electrons
• Each p subshell holds at most 6 electrons
• Each d subshell holds at most 10 electrons
• Each f subshell holds at most 14 electrons

There can only be a max of 2 electrons per orbit, so the p subshell would need 3 orbitals, each with 2 electrons. d subshell would need 5 orbitals, each with 2 electrons. f subshell would need 7 orbitals, each with 2 electrons. Sometimes an orbital will only have one electron is there is an odd number of electrons. 

 1s²2s² 2p⁶3s² 3p⁶4s² 3d¹⁰ 4p⁶5s² 4d¹⁰ 5p⁶6s² 4f¹⁴ 5d¹⁰ 6p⁶7s² 5f¹⁴ 6d¹⁰ 7p⁶

Above is the order in which electrons are filled. For example, a neutral oxygen atom has 8 electrons, so the electron configuration would be:

1s² 2s² 2p⁴ 

^{Notice that the p only has a 4, and not a 6. This is alright. The superscripts should add up to the number of electron in the atom. In this case, it adds up to 8, which is correct.} 

When writing electronic configurations for negative ions, simply add the appropriate number of electrons from where the neutral atom left off. 

When writing electronic configurations for positive ions, take away electrons from the outermost shell first. (aka. the higher energy shell/larger n-value) 

Another method of writiting configurations is Core Notation.

The core is the part of the configuration of the nearest noble gas that comes before the given element. (Ex/ Ar is the noble gas that comes before Br)

The outer part consists of all the electrons outside of the core. 

The core notation for Rubidium would be... [Kr]5s^1 

Do you see how all the numbers and letters that should've been before 5s^1 was replaced by Kr? 

Another example... the core notation for Chlorine would be... [Ne]3s^2 3p^5 

Electron configuration can also tell me the number of valence electrons that an atoms has. Valence electrons are electrons in the outermost open shell. By open, we mean that the shell contains less than its maximum number of electrons. Whereas, a closed shell is a shell containing exactly its max number of electrons.

In electron configuration, valence electrons are those that aren't in the core, or in d- and f- subshells.

Ex/ Determine number of valence electrons by looking at core notation of Selenium.

[Ar] 4s^2 3d^10 4p^4

There are 6 valence electrons because of the 4s^2 and the 4p^4 part of the configuration. 3d^10 doesn't count because its a d- subshell.

Atomic Structure

Protons and Neutrons are both located in the nucleus, and weigh about the same. The weight of the protons and neutrons make up the atomic mass.

Electrons are located in a cloud around the nucleus, floating in their orbits. Electrons weigh almost zero.

The number of protons (positive) and electrons (negative) are the same in a NEUTRAL atom. The number of protons is the atomic number, so if a proton is added, a new element would be formed.

If an atom has a charge, meaning the number of protons and electrons AREN'T the same, then it is called an ION. Atoms that have gained or lost electrons become ions.

ANION: a negatively charged ion, meaning it GAINED elections. (non-metals gain electrons)

CATION: a positively charged ion, meaning it LOST electrons. (metals tend to give away electrons)

The mass number is the total number of protons + neutrons.

The atomic mass of the periodic table is the average mass of an elements isotopes. The atomic mass should be close to the mass number.

If a NEUTRON is added to an elements nucleus, then a heavier version of the SAME element is formed. This is called an ISOTOPE.

So to review:

When a proton is added, a new ELEMENT is formed.

When a neutron is added, an ISOTOPE is formed.

Let's move on the natural mixtures. There can not be half of a proton/neutron, so when the periodic table states that the atomic mass of chlorine is 35.5, we know that it must be the average mass of the isotopes.

When given the percentage of each isotope in a mixture, and a precise mass for each of those isotopes, we can calculate the average mass of it. This can be done simply by multiplying the percentage and the mass of each, and adding the products together.

Ex/ Given the following information, calculate the average mass of this oxygen mixture.

Oxygen-16: 99.763%, 15.99491463g
Oxygen-17: 0.038%, 16.9991312g
Oxygen-18: 0.020%, 17.9991603g

0.99763 x 15.99491463  = 15.9570067 g
0.00038 x 16.9991312 = 0.00645967 g
0.00020 x 17.9991603 = 0.003599832 g

Now add all the products together to get your average mass:

15.9570067 + 0.00645947 + 0.004599832 = 15.967 g 

Atomic Theory

A long time ago, Greek philosophers believed that all matter was made of atoms, which was the smallest piece of matter.

Aristotle believed that matter was made of combinations of earth, fire, water, and air. That led Alchemists to experiment with matter to try to turn common metals into Gold.
Aristotle's 4-element theory lasted for about 2000 years! However, it was not a scientific theory because it could not be tested.

Here are some significant scientists who studied the atom:

Democritus: A greek philosopher who believed that atoms were indivisible spheres that could not be seen with the naked eye.

Lavoisier: Discovered conservation of mass, and the law of definite proportions.

Proust: Discovered that if a compound is to be broken down, that the products would exist in the same ratio as the original compound- proving Lavoisier's laws.

Dalton: Still believed that atoms were solid indestructible spheres, but states that every element has a different type of atom. Stated that atoms of one type of element can combine with the atoms of another to form chemical compounds, and that atoms cannot be created nor destroyed.

JJ Thomson: Created the "raisin bun" model: solid positive spheres, with negative particles embedded within. This was the first atomic theory to have positive and negative charges! He used the cathode tube experiment to demonstrate the existence of electrons.

Rutherford: Showed the atoms have a dense positive center (nucleus), with electrons outside of it. He discovered this with the gold leaf experiment, which resulted in the planetary model of the atom. It explains the reason why electrons spin around the nucleus. It also suggested that atoms were mostly empty space.

Niels Bohr: Studied gaseous samples of atoms, which glowed when an electric current passed through them. Niels Bohr proposed that electrons surround the nucleus in different energy levels, and can jump from one to another.

Of course, now we know that the modern atom is made of three kinds of particles called SUBATOMIC particles, which include:

PROTONS (+)
NEUTRONS (neutral)
ELECTRONS (-)

The atom on the left is what scientists thought they looked like- solid indivisible spheres. This changed when JJ Thomson discovered the existence of protons and electrons! 

On the right is the modern atom. 

PERCENT YIELD YES I'M TYPING IN CAPS.

Hi there.
Imagine if you had a bag of chips. Yes I just made you hungry. I bet 50% of you just went into the kitchen to check if you had chips. Anyways, back to my point. Imagine the bag is big, and by big, I don't mean those baby bags you find in vending machines. By big, I mean momma sized chips, like them big ones you get in Costco. Appealing, I know. Would you be able to finish them? Perhaps some of you could, but most of you most likely can't without getting heartburn. This is the same with chemical reactions; sometimes not all of the reactants or products get used up; they can only do so much. What if we wanted to know how much of the compound was used up? (or how much of the bag of chips we finished) Thus now, ladies and germs, I present to you the PERCENT YIELD.


And yes I'm aware the chip explanation was uncalled for. But it's a good analogy no?

Percent Yield can be generally calculated using this formula:
Percent Yield= mass of product actually formed
                        --------------------------------------------------     x 100%
                        mass of product expected to be formed
This formula is actually not necessary when you use logic. It is like calculating a test mark. When you calculate a test mark, you divide what you got, by what you possibly could've gotten. Ahhhh logic feels good when you use it, doesn't it?

Here are a few examples:
EX/ What is the percent yield for a reaction if you predicted the formation of 21. grams of C₆H₁₂ and actually recovered only 3.8 grams?
-21g is expected, but you only got 3.8 grams. Bummer.
You would figure it out like so:    (3.8g/21g)x 100% = 18% (don't forget sig figs)


Now that was easy, wasn't it?
Now here, I will throw a curve ball at your way.


EX/ Consider the reaction: U+3Br2--> UBr6. What is my actual yield of uranium hexabromide if I start with 100 grams of uranium and get a percent yield of 83%?
First, we would use basic stoichiometry calculations to figure the amount of uranium hexbromide that is expected. Like so:
100g U x  1 mol Mg  x   1 mol H2   x 2.0g 
                --------------     -------------     ------------   = 301.4g (don't round yet! This is NOT your final ans)
                24.3g Mg       1 mol Mg     1 mol H2 


Since we know 2 variables (percent yield and expected amount), Let x= actual produced amount.
   x/301.4g=0.83. Therefore, x=250g=200g (S.F.)


DID THAT BEND YOUR MIND OR WHAT?!
Yes I know I'm an enthusiastic person when it comes to chemistry.


So long, young disciples.

^GG is all I have to say to that.