Thursday, December 30, 2010

Mole Concept # 2







Group 8
Carbonel
Catapang
Chua
Cornelio
Dumpit
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Wednesday, December 29, 2010

Binary Compounds

Binary Compounds

Chemical compound that contains exactly two different elements


Binary Ionic Compounds

-Compounds in which two types of ions (metal cation and nonmetallic anion) combine to form a ionic compound
-Examples are Calcium chloride (CaCl2), sodium fluoride (NaF), and magnesium oxide (MgO),

Two types of Binary Ionic Compounds
Type 1: The binary ionic compound in which cation can has only one form (charge), like Na+, Mg+2 and Al+3.
Few examples of type 1 binary ionic compounds are as, NaCl, KBr, LiF, CaI2, AlF3, MgBr2 etc.
Type 2: The binary ionic compound in which cation can have the multiple forms (charge), like Fe+2 and Fe+3
Examples of type 1 binary ionic compounds are as FeCl2 and FeCl3, AgCl and AgCl2.

How to name Binary Ionic Compounds

1. Metal (Cation) + NonMetal (anion) –ide

Example:

NaCl
Na – Sodium
Cl – Chlorine

Sodium + Chlorine –idea = Sodium Chloride

2. Use of –ous and –ic

-ous = lower one
-ic = higher one

Example:

FeCl2 and FeCl3

FeCl2 = Ferrous Chloride or Iron (II) Chloride
FeCl3 = Ferric Chloride or Iron (III) Chloride


Binary Covalent Compounds
-Made from two nonmetal elements. In binary covalent compound sharing of electrons takes place.
-Examples of binary covalent compounds are:  N2O, P2O5, N2H4, CH4 and H2O.

How to name Binary Covalent Compounds

1.Prefix + Nonmetal  +  Prefix +nonmetal-ide

List of Prefix:



Example:

N2H4

Di- nitrogen  +   Tetra- hydrogen –ide

= Dinitrogen Tetrahydride


2.      Use of –ous and –ic

-ous = higher
-ic = lower


SOURCES: 
http://www.tutorvista.com/chemistry/binary-compounds-list

http://www.files.chem.vt.edu/RVGS/ACT/notes/Nomenclature.html

http://faculty.sdmiramar.edu/fgarces/zCourse/All_Year/Ch100_OL/aMy_FileLec/04OL_LecNotes_Ch100/05_CompoundBonding/501_IonicCompounds/501_IonicCompounds.htm

http://en.wikipedia.org/wiki/Binary_ionic_compound


GROUP 2: 

Marquez
Lacanilao
Lagaya
Manacsa
Legazpi
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Tuesday, December 28, 2010

Moles



A mole is defined as the number or quantity of a certain substance that has the same measurement of particles as are found in a 12 gram carbon gaining a -12. It follows the number 6.02x1023 or also known as Avogadro’s number. This states that one mole of a certain element or compound contains 6.02x1023 molecules of the given compound. 


Calculating the Moles of a compound

(1) Ca - 40.08 – 40.08             In the compound CaCO3, there are 3 different
(1) C - 12.01 – 12.01               elements namely, Calcium (Ca), Carbon (C), 
(3) O - 16. 00 – 48.00              and Oxygen (O). There are 3 O, 1 C, & 1 Ca. 
                          -------              By getting the mass of each element, we 
                      100.09 u             can calculate their mass in Moles. 1 Ca 
                        CaCO3                weighs 40. 08, 1 C weighs 12.01, & 3 O's 
                                                                 weigh 48.00,having 100.09 u or mol CaCO3. 

100. 09 g/mol CaCO3


Mole to Mass, Mass to Mole


If you want to change the measurement of a certain compound to mole to mass, just change u or mol to g/mol and vise versa for mass to mole.




Exercises
     Calculate the moles of the following compounds and express your final answer with the unit g/mol (unit for mass):


          1. Bi2O3
          2. FeSO4
          3. Ca (CH3COO)2
          4. (NH4)2Cr2O7
          5. AgNO3
          6. Mg (ClO)2
          7. Zn (IO4)2
          8. CH3 (CH2)3 COF
          9. CaSO4
          10. CuCl2

Group 7
Encarnacion
Evangelista
Fernandez
Isaac
Jayco

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Friday, October 1, 2010

Periods, Groups, Families, 
& Valence Electron



1
H		 2
He
3

Li		 4

Be		 5

B		 6

C		 7

N		 8

O		 9

F		 10

Ne
11

Na		 12

Mg		 13

Al		 14

Si		 15

P		 16

S		 17

Cl		 18

Ar
19

K		 20

Ca		 21

Sc		 22

Ti		 23

V		 24

Cr		 25

Mn		 26

Fe		 27

Co		 28

Ni		 29

Cu		 30

Zn		 31

Ga		 32

Ge		 33

As		 34

Se		 35

Br		 36

Kr
37

Rb		 38

Sr		 39

Y		 40

Zr		 41

Nb		 42

Mo		 43

Tc		 44

Ru		 45

Rh		 46

Pd		 47

Ag		 48

Cd		 49

In		 50

Sn		 51

Sb		 52

Te		 53

I		 54

Xe
55

Cs		 56

Ba		 * 72

Hf		 73

Ta		 74

W		 75

Re		 76

Os		 77

Ir		 78

Pt		 79

Au		 80

Hg		 81

Tl		 82

Pb		 83

Bi		 84

Po		 85

At		 86

Rn
87

Fr		 88

Ra		 ** 104

Rf		 105

Db		 106

Sg		 107

Bh		 108

Hs		 109

Mt		 110

Ds		 111

Rg		 112

Cn		 113

Uut		 114

Uuq		 115

Uup		 116

Uuh		 117

Uus		 118

Uuo

57

La		 58

Ce		 59

Pr		 60

Nd		 61

Pm		 62

Sm		 63

Eu		 64

Gd		 65

Tb		 66

Dy		 67

Ho		 68

Er		 69

Tm		 70

Yb		 71

Lu
89

Ac		 90

Th		 91

Pa		 92

U		 93

Np		 94

Pu		 95

Am		 96

Cm		 97

Bk		 98

Cf		 99

Es		 100

Fm		 101

Md		 102

No		 103

Lr




Alkali Metal Alkaline Earth Basic Metal


Halogen		 Noble Gas Non
Metal
Rare Earth Semi-Metal Transition Metal


Periods
The elements in rows are called as periods. A sequence of elements arranged in order of increasing atomic number and forming one of the horizontal rows in the periodic table.  The period number of an element signifies the highest unexcited energy level for an electron in that element. The number of elements in a period increases as you move down the periodic table because there are more sublevels per level as the energy level of the atom increases. It ranges from period 1 until period 7.


Note: All of the elements in a period have the same number of atomic orbitals.

Groups
In chemistry, it is considered to be a set of chemical elements in the same vertical column of the periodic table. The elements in a group have similarities in the electronic configuration of their atoms, and thus they exhibit somewhat related physical and chemical properties. They are composed of group IA, IIA, IIIB, IVB, VB, VIB, VIIB, VIIIB, VIIIB, VIIIB, IB, IIB, IIIA, IVA, VA, VIA, VIIA, VIIIA.


Note: The group number of an element is equal to its valence electron.


Families
Families are groups of elements with similar chemical properties. In the periodic table of elements, a family is a vertical column which is alike as the groups. Each group has a corresponding family:



  • Group IA - Alkali Metals
  • Group IIA - Alkaline Earth Metals
  • Group IIIB - Early Transition Metals 
  • Group IVB - Early Transition Metals
  • Group VB - Early Transition Metals
  • Group VIB - Early Transition Metals
  • Group VIIB - Early Transition Metals
  • Group VIIIB- Late Transition Metals
  • Group IB - Late Transition Metals
  • Group IIB - Late Transition Metals
  • Group IIIA - Boron
  • Group IVA - Carbon
  • Group VA- Nitrogen
  • Group VIA - Oxygen
  • Group VIIA- Halogens
  • Group VIIIA - Noble Gases



Valence Electron
The valence electrons are the electrons in the last shell or energy level of an atom. They do show a repeating or periodic pattern. The valence electrons increase in number as you go across a period. Then when you start the new period, the number drops back down to one and starts increasing again. 


Note: Number of Valence electrons = Group Number




Exercises
I. PERIODS:
1. There are __ periods in the Periodic Table of Elements
2. Elements in a period are arranged from left to right by increasing ______ ______.
3. The elements Tantalum and Osmium can be found on which period?
4. Vanadium and Calcium are on the same period. True or False?
5. Give 3 elements that can be found on the 6th period.


II. GROUPS:

1. There are __ groups in the Periodic Table of Elements
2. Groups are horizontal rows of elements on the Periodic Table. True or False?
3. The elements Aluminum and Indium can be found on the __th group.
4. Oxygen and Polonium can be found on the same group. True or False?
5. The group number of an element is equal to its _______ ________.


III. FAMILIES:

1. A family is a _____ of elements with the same chemical properties.
2. What is the family name of Group IVA?
3. Lithium and Strontium are located on the same family. True or False?
4. Give 3 elements from the Chalcogens family.
5. How many elements can be found in the Alkali Metals family?


IV. VALENCE:
1 - 5. Give the valence of an element that has an atomic number of 3, 20, 31, 17 & 8.


V: ALL FOUR TOPICS:
1-5. Give the Period, Group, Family, & Valence of an element that has an atomic number of 19, 33, 5, 12, and 36 without look at the periodic table.


Members
  • Encarnacion, Carol
  • Evangelista, Kaira
  • Fernandez, Gaby
  • Isaac, Bianca
  • Jayco, Christelle




Reference
http://chemistry.about.com/library/blperiodictable.htm
http://www.thefreedictionary.com/period
http://www.chem4kids.com/files/elem_pertable.html
http://www.britannica.com/EBchecked/topic/247062/group
http://www.thefreedictionary.com/family
http://dl.clackamas.cc.or.us/ch104-06/valence_electrons.htm
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IONIZATION & ELECTRON AFFINITY
group five



CLICK `EM ALL!

PhotobucketPhotobucketPhotobucketPhotobucket

ATTENTION
Hello, dear Two Five-rs and Sir De Leon.
Please be informed that the first 'videos' button is for the video about Electron Affinity and the second 'videos' is for the video about Ionization energy.

GROUP FIVE ; TWO FIVE
RODRIGUEZ, Angela
ROSADIA, Rachel
SEVALLA, Janine
SOLIS, Maacah
TAN-PALANCA, Patricia
TRINIDAD, Irene
CNs 31 - 36
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Thursday, September 30, 2010

IONIC BONDING
  • Chemical Bond formed between 2 oppositely charged ions by the transfer of electrons.
  • Involves a metal and a non metal element
  • The farther two elements are across the periodic table; the more likely they are to form an ionic compound



Sodium  (on the left) loses its one valence electron to chlorine who has 7 valence electrons (on the right),




The Result is.. 

 A positively charged sodium ion (left) and a negatively charged chlorine ion (right).


NOTE: Chlorine became negatively charged because it gained an electron which has a negative charge. And Sodium became postively charged because it has more protons+ than electrons-



ILLUSTRATION



USING LEWIS ELECTRON DOT SYSTEM



Element Pair

             Lithium has 2 valence electrons .









Chlorine has 7 valence electrons 

 









Electron Transfer








Lewis Structure




The Ionic Compound






Covalent Bonding

  • Sharing of one or more pairs of electrons between atoms, in order to produce a mutual attraction


  •       Covalent bonding occurs because the atoms in the compound have a similar tendency for electrons (generally to gain electrons).


  •       This most commonly occurs when two nonmetals bond together. Because both of the nonmetals will want to gain electrons, the elements involved will share electrons in an effort to fill their valence shells



  •       Neither atom completely loses or gains electrons as in ionic bonding

There are two types of covalent bonding:
1. Non-polar bonding
2. Polar bonding




Nonpolar Covalent Bonding

  • A nonpolar covalent bond is formed when an element has an equal attraction or affinity for electrons

  • It is also formed whenever two atoms of the same element bond together.

  • The H2 molecule is a good example of the first type of covalent bond, the non-polar bond. 











Polar Covalent Bonding







  • When electrons are unequally shared between two atoms, a polar covalent bond is formed

  • it also occurs when one atom has a stronger affinity for electrons than the other.
    • A good example of a polar covalent bond is the hydrogen-oxygen bond in the water molecule.








  • IMPORTANT TERMS!!





          - Single covalent bond
    It is the sharing of a single pair of electron between bonded atoms. 


    -          Double covalent bond
    Shares 2 electron pairs


    -          Triple covalent bond
    Shares 3 electron pairs


    -          Bonding electrons
    Electrons shared between the 2 atoms


    -          Lone Pairs
    Valence electron pairs that are not involved in bonding



    GROUP 8
    CHUA
    CORNELIO
    DUMPIT 
    CATAPANG
    CARBONEL
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