Bonding Habits
We learned that by looking at the periodic table you could detemine weather or not an atom is a metal or a non-metal Be is a metal. Also we learned that metals form positive ions which means that it loses electrons as in Be it loses 2 electrons making its charge +2. In addition, if an atom is a non-metal then it gains electrons as in He it gains 1 electron making its charge -1. You can determine the amount of electrons an atom will be gaining/losing by looking at the periodic table or an electron configuration. We can also find the charge of an atom by comparing the amount of electrons and protons after the atom has formed an ionic bond.
Ionic Compounds
We learned how to predict the formula of an ionic compound. First you find the charges of the ions by them already being their or you have to find that atom on the periodic table and finding its charge when it forms an ion. Then, your goal is to make the charge of the ionic bond zero. To do this you need to either double one of the ions or find the least common dinominator. Then you write it positive ion then negative ion. Ex. K+ and O2- you want to make their overall charge zero so you have -2 from K so to even that out with a + you simply just make it K2 making the formula k2O. A more challenging problem would be when you have to add a sub number to both the positive and negative ions. Ex. Fe3+ and CO32- in order to find the formula for this ionic compound you must find the least common dinominator which in this case is 6 so you would need two Fe3+ and three CO32-. The answer for this would be 2Fe(Co3)3. You need parentheses for the Co3 because that is the original ion and you don't want to get confused with how many of that ion you need to make the ionic bond come out to zero so you NEED the perentheses. In some problems you are not going to have the charges given to you so you need to look at your periodic table and find out if the ion is positive or negative and how many electrons does it gain or lose.
Then you resume the original process. Ex. K and S K's charge is +1 and S's charge is 2-. So you need to K's to even out the one S so the formula would be this K2O.
Peter I
Ionic
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Period 2 Chemistry 2010
Thursday, October 28, 2010
Wednesday, October 13, 2010
10.13.10
Metal Reactivity: Periodic Trends Lab
What we did today:
First We watched videos on how the Alkali Earth metals [Lithium, Sodium, Potassium, Rubidium, Cesium, and Francium(Francium excluded because it is illegal to obtain)] react with water. These were their reactions...
Li- Floats gives off H2 gas in reaction to water
Na- Similar reaction to water as Lithium ,but reacts more vigorously
K- Gives off flame with reaction to water
Rb- Similar to potassium ,but more violent
Cs- Cesium gives off a violent explosion with reaction to water
After the videos we were asked what trend that might be noticed as we go farther down the Alkali earth family column and the answer was they were more violent in reacting with water.
Next we were ask to describe the appearences of magnesium and aluminum.
Mg- Dull strip of metal
Al- Thin metal sheet
We were then asked what happens when they are ignited.
Mg- Sparkles with a blinding white light
Al- Shrivles
Todays Lab:
In todays lab we repeated what we saw previously in the day(combining the Alkali earth metals with water). Your data table should have similar if not the same information as the the data you collected from watching the video previous in the class period.
Post Lab Questions: (Answers)
1. Is a shiny metal more or less reactive? (Shiny metals are less reactive)
2. Which metal was most reactive in the air? (Calcium)
3. Rank the metals in order of most reactive with water to least reactive. (Ca,Al,Mg)
4. Which metal reacted to produce the most OH ions? (Calcium)
5. Rank the metals in order of most reactivity with water to least reactivity with HCl. N/A
6. Rank the four metals in this lab from the most reactivity to the least reactivity. (Ca,Al,Mg)
7. What can you conclude about the reactivity of metals as you move down a column or group? (Reacts more vigorously).
8. What can you conclude about the metals as you go across the periodic table? (More reactive)
9. N/A
Don't forget to look at your schedule to see what the homework is.
That concluded the day and the next scriber will be Brandon
PLEASE COMMENT
Wednesday, October 6, 2010
October 6, 2010
Electron Configuration
In class today we learned more about how to find the electron configuration of a nuetral atom. The point of electron configuration is to find the location of the electron.
Shapes of Orbitals
There are four different shapes of orbitals
1) S-one orientation-holds 2 electrons
2)P-three orientations-holds 6 electrons
3)D-five orientations-holds 10 electrons
4)F-seven orientations-holds 14 electrons
The S block always starts as 1S
The P block always starts with 2P
The D block always starts with 3D
The F block always starts with 4F
EXAMPLE 1: If the electron configuration of a neutral atom is 1s2 2s2 2p6 3s2 3p6 then....
a)How many electrons does it have?
18 electrons
(there are two ways in how to find this)
18 protons
(Since this is a neutral atom, the electrons and the protons are the same amount)
c)Write the symbol for this atom
Ar
(You can find this on your periodic table)
EXAMPLE 2: Lets say you need to write the electron configuration of Bi (Bismuth). You have to start with 1s2 and end with 6p3(which is where bismuth is located) The way to find write the in between atoms is to read the periodic table from left to right.
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p2.
Orbital Diagram
Each half arrow represents how many atoms are in that row.
ALWAYS PUT ONE HALF ARROW FIRST IN EACH BOX BEFORE PUTTING THE SECOND HALF ARROW IN IT.
Ionic Electron Configuration
To write the ionic electron configuration is same as usual. Except for example if they want you to write the electron configuration of O-2, then you have to find where O is, which is 2p4, and go forward 2 because you are gaining 2 more electrons, which is 2p6 and is the atom Ne (Neon)
IN CLASS
We did pages 6, 7 and some of 11 of electron configuration.
REMINDERS
Webassigns are due on Friday. Test is on Friday.
HOMEWORK
Page 8 of electron configuration.
In class today we learned more about how to find the electron configuration of a nuetral atom. The point of electron configuration is to find the location of the electron.
Shapes of Orbitals
There are four different shapes of orbitals
1) S-one orientation-holds 2 electrons
2)P-three orientations-holds 6 electrons
3)D-five orientations-holds 10 electrons
4)F-seven orientations-holds 14 electrons
The S block always starts as 1S
The P block always starts with 2P
The D block always starts with 3D
The F block always starts with 4F
EXAMPLE 1: If the electron configuration of a neutral atom is 1s2 2s2 2p6 3s2 3p6 then....
a)How many electrons does it have?
18 electrons
(there are two ways in how to find this)
- Add all of the second numbers together (2+2+6+2+6)
- Look at the last electron configuration, which is 3p6, and find it on your periodic table.
18 protons
(Since this is a neutral atom, the electrons and the protons are the same amount)
c)Write the symbol for this atom
Ar
(You can find this on your periodic table)
EXAMPLE 2: Lets say you need to write the electron configuration of Bi (Bismuth). You have to start with 1s2 and end with 6p3(which is where bismuth is located) The way to find write the in between atoms is to read the periodic table from left to right.
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p2.
Orbital Diagram
Each half arrow represents how many atoms are in that row.ALWAYS PUT ONE HALF ARROW FIRST IN EACH BOX BEFORE PUTTING THE SECOND HALF ARROW IN IT.
Ionic Electron Configuration
To write the ionic electron configuration is same as usual. Except for example if they want you to write the electron configuration of O-2, then you have to find where O is, which is 2p4, and go forward 2 because you are gaining 2 more electrons, which is 2p6 and is the atom Ne (Neon)
IN CLASS
We did pages 6, 7 and some of 11 of electron configuration.
REMINDERS
Webassigns are due on Friday. Test is on Friday.
HOMEWORK
Page 8 of electron configuration.
Sunday, October 3, 2010
October 1, 2010
ATOMIC STRUCTURE: In class on Friday we defined a few terms that have to do with atoms.
Proton- It has a positive charge and its location is in the nucleus (Remember Proton is Positive)
Neutron- Neutral, it has no charge. Its location is in the nucleus as well.
Electron- Located outside the nucleus. They have a negative charge
We also learned some stuff that has to do with the PERIODIC TABLE.
-The number located above the element's symbol is the atomic number. It represents the number of protons
-The number below the symbol is the atomic mass. That stands for the number of protons PLUS the number of neutrons.
*An atom will usually have the same number of protons and electrons. When those numbers are the same, it has no charge. The only way an atom can get a positive or negative charge is by losing or gaining electrons.
EXAMPLE:
Oxygen's atomic number is 8. Therefore it has 8 protons as well as 8 neutrons. If oxygen were to GAIN 2 electrons(making its total 10 electrons), then it would have a -2 ion(charge) because it has two more electrons than protons. On the other hand, if it were to LOSE two electrons (making its total electrons be 6), then it would have a +2 ion because it has two more protons.
ATOMIC MODELS:
We learned some stuff about orbitals and relative energy and other stuff with Bohr's model, but I did not quite undestand much of that thus, I would explain it poorly. Please be sure to ask Mr. Paek about that stuff.
FIREWORKS LAB:
The purpose was to observe the recations of 7 different salts when they were exposed to fire.
PRE LAB: When electrons drop down an energy level, they give off a specific amount of energy. The energy hits our eyes, excities our neurons, and then we see color.
QUESTION: What does the term "electrons becoming excited" mean?
ANSWER: Energy is added to the electrons so they jump energy levels.
Materials: 7 salts, sticks, water, Bunsen Burner.
Procedure: 1.First we wet the stick a bit in the water
2. Then we dipped it in the salt
3. We placed it over the Bunsen Burner (while it was lit) and observed the reaction
4. Then recorded it in our table
Results:
Proton- It has a positive charge and its location is in the nucleus (Remember Proton is Positive)
Neutron- Neutral, it has no charge. Its location is in the nucleus as well.
Electron- Located outside the nucleus. They have a negative charge
We also learned some stuff that has to do with the PERIODIC TABLE.
-The number located above the element's symbol is the atomic number. It represents the number of protons
-The number below the symbol is the atomic mass. That stands for the number of protons PLUS the number of neutrons.
*An atom will usually have the same number of protons and electrons. When those numbers are the same, it has no charge. The only way an atom can get a positive or negative charge is by losing or gaining electrons.
EXAMPLE:
Oxygen's atomic number is 8. Therefore it has 8 protons as well as 8 neutrons. If oxygen were to GAIN 2 electrons(making its total 10 electrons), then it would have a -2 ion(charge) because it has two more electrons than protons. On the other hand, if it were to LOSE two electrons (making its total electrons be 6), then it would have a +2 ion because it has two more protons.
ATOMIC MODELS:
We learned some stuff about orbitals and relative energy and other stuff with Bohr's model, but I did not quite undestand much of that thus, I would explain it poorly. Please be sure to ask Mr. Paek about that stuff.
FIREWORKS LAB:
The purpose was to observe the recations of 7 different salts when they were exposed to fire.
PRE LAB: When electrons drop down an energy level, they give off a specific amount of energy. The energy hits our eyes, excities our neurons, and then we see color.
QUESTION: What does the term "electrons becoming excited" mean?
ANSWER: Energy is added to the electrons so they jump energy levels.
Materials: 7 salts, sticks, water, Bunsen Burner.
Procedure: 1.First we wet the stick a bit in the water
2. Then we dipped it in the salt
3. We placed it over the Bunsen Burner (while it was lit) and observed the reaction
4. Then recorded it in our table
Results:
- Li+(Lithium) Gave off a hot pink color
- Na+(Sodium) Gave off a orange color that looked like fire
- K N O3 Gave off a dull green
- K Cl Gave off a dull purple
- Sr2+ (Strontium) Was red orange
- Cu(Copper) gave off a very dull green (almost white looking)
And Cu2+ was an emerald green
At the end we has three "mystery salts" and had to figure out which ones they were based on the results of the colors we got.
Postlab:
Why did each metal salt give off a different color? That's because they had different numbers of electrons and they each went to different energy levels.
NEXT SCRIBEPOST WILL BE: Zak
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