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Broughton High School
Student Workbook Physical Science – Chemical Bonding-“Chapter 20” Mr. Davis
Name: _________________________________________ Section ___
Chemical Bonding
Chapter 20
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Chemical Bonding: Student Workbook for Physical Science, Schemes and Mind Maps of Chemistry
Physical Science – Chemical Bonding-“Chapter 20”. Mr. Davis. Practice Counting Atoms Worksheet. Directions for each problem. 1. Write down the different ...
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Broughton High School
Name: _________________________________________ Section ___
Chemical Bonding
Chapter 20
Broughton High School
Chapter 20 – Chemical Bonding Vocabulary Words
Vocabulary Word (^) Definition
1. Binary Compound
2. Chemical Bond
3. Chemical Formula
4. Covalent Bond
5. Hydrate
6. Ion
7. Ionic Bind
8. Molecule
9. Non Polar Molecule
10. Oxidation Number
11. Polar Molecule
12. Polyatomic Ion
The Lewis Theory: Valence electrons , or the electrons in the outermost electron shell, have an essential role in chemical bonding. Ionic bo nds are formed between atoms when electrons are transferred from one atom to another. Ionic bond is a bond between nonmetals and metals. Covalent bonds are formed between atoms when pairs of electrons are shared between atoms. A covalent bond is between two nonmetals. Electrons are transferred/shared so that each atom may reach a more stable electron configuration i.e. the noble gas
configuration which contains 8 valence electrons. This is called octet rule.
Broughton High School Elements and their Symbols
Directions : write the symbols for the following elements.
- Oxygen ________________ 21. Xenon ________________
- Hydrogen ________________ 22. Arsenic ________________
- Chlorine ________________ 23. Gallium ________________
- Sodium ________________ 24. Chromium ________________
- Fluorine ________________ 25. Cobalt ________________
- Carbon ________________ 26. Krypton ________________
- Nitrogen ________________ 27. Vanadium ________________
- Helium ________________ 28. Aluminum ________________
- Copper ________________ 29. Mercury ________________
- Sulfur ________________ 30. Tin ________________
- Magnesium ________________ 31. Boron ________________
- Manganese ________________ 32. Nickel ________________
- Neon ________________ 33. Cadmium ________________
- Bromine ________________ 34. Beryllium ________________
- Silver ________________ 35. Polonium ________________
- Lead ________________ 36. Uranium ________________
- Iron ________________ 37. Cesium ________________
- Calcium ________________ 38. Strontium ________________
- Potassium ________________ 39. Palladium ________________
- Gold ________________ 40. Barium ________________
Directions : Write the name of the element that corresponds to each of the following symbols.
- Cu ________________ 54. Sb ________________
- K ________________ 55. In ________________
- C ________________ 56. Ta ________________
- Au ________________ 57. Ce ________________
- Zn ________________ 58.Nb ________________
- Pb ________________ 59. I ________________
- At ________________ 60. In ________________
- Bi ________________
- W ________________
- Y ________________
- Mo ________________
- Rh ________________
- Zr ________________
Broughton High School
Broughton High School Number of Atoms in a Formula
Directions: Determine the number of atoms in the following chemical formulas.
- NaCl ________________________________________________________________
- H 2 SO 4 ________________________________________________________________
- KNO 3 ________________________________________________________________
- CaCl 2 ________________________________________________________________
- C 2 H 6 ________________________________________________________________
- Ba(OH) 2 ________________________________________________________________
- NH 4 Br ________________________________________________________________
- Ca 3 (PO 4 ) 2 ________________________________________________________________
- Al 2 (SO 4 ) 3 ________________________________________________________________
- Mg(NO 3 ) 2 ________________________________________________________________
- Cu(NO 3 ) 2 ________________________________________________________________
- KMnO 4 ________________________________________________________________
- H 2 O 2 ________________________________________________________________
- H 3 PO 4 ________________________________________________________________
- (NH 4 ) 3 PO 4 ________________________________________________________________
- Fe 2 O 3 ________________________________________________________________
- NaC 2 H 3 O 2 ________________________________________________________________
- Mg(C 2 H 3 O 2 ) 2 ________________________________________________________________
- Hg 2 Cl 2 ________________________________________________________________
- K 2 SO 3 ________________________________________________________________
Hint:
Coefficients:
Coefficients apply to the entire compound. You multiply the coefficients and the subscripts.
Example : 2 H 2 S
Atoms of Hydrogen = (2 X 2) = 4
Atoms of Sulfur = (2 X 1) = 2
Total Atoms equals = 6 atoms
If there isn’t a subscript behind an element, there is only one atom of that element.
Broughton High School Practice Counting Atoms Worksheet
Directions for each problem
1. Write down the different elements in each compound.
2. Write down how many of that particular atom there are
3. How many atoms are there total in the compound.
Examples:
A) MgCl 2 Mg – 1 B) 5 ZnSO4 Zn – 5
Cl – 2 S – 5
3 total O – 20
30 total
1) NaOH ______________ 2) 4 HNO 3 ______________ 3) MgCl 2 ______________
4) 4 Li 2 O ______________ 5) 2 NaOH ______________ 6) Li 2 SO 4 ______________
7) 3 H 2 O ______________ 8) NaC 2 H 3 O 2 ______________ 9) 3 Al 2 O 3 ______________
10) NH 4 Cl ______________ 11) 5 ZnSO 4 ______________ 12) 7 C 2 S 2 ______________
SUPER STAR CHALLENGE!
13) 2 Sr 3 (PO 4 ) 2 ______________ 14) 4 Al(OH) 3 ______________ 15) Ca (C 2 H 3 O 2 ) 2 ______________
16) 4 Al 2 (SO 3 ) 3 ______________ 17) 2 (NH 4 ) 3 PO 4 ______________ 18) 4 Mg(OH) 2 ______________
Broughton High School
Types of Chemical Bonds
Ionic Bonds
The ionic bond is formed by the attraction between oppositely charged ions. Ionic bonds are formed between metals and
nonmetals. Remember that metal atoms lose one or more valence electrons in order to achieve a stable electron
arrangement. When a metal atom loses electrons it forms a positive ion or cation. When nonmetals react they gain one or
more electrons to reach a stable electron arrangement. When a nonmetal atom gains one or more electrons it forms a
negative ion or anion. The metal cations donate electrons to the nonmetal anions so they stick together in an ionic
compound. This means that ionic bonds are formed by the complete transfer of one or more electrons.
Covalent Bond
A covalent bond is formed between nonmetal atoms. The nonmetals are connected by a shared pair of valence electrons.
Remember, nonmetals want to gain valence electrons to reach a stable arrangement. If there are no metal atoms around to
give them electrons, nonmetal atoms share their valence electrons with other nonmetal atoms. Since the two atoms are
using the same electrons they are stuck to each other in a neutral particle called a molecule. A molecule is a neutral
particle of two or more atoms bonded to each other. Molecules may contain atoms of the same element such as N 2 , O 2 ,
and Cl 2 or they may contain atoms of different elements like H 2 O, NH 3 , or C 6 H 12 O 6. Therefore, covalent bonding is found
in nonmetallic elements and in nonmetallic compounds. Covalent bonds are intramolecular forces; that is, they are inside
the molecule and hold the atoms together to make the molecule. Covalent bonds are strong bonds and it is difficult and
requires a lot of energy to break a molecule apart into its atoms. However, since molecules are neutral one molecule does
not have a strong electrical attraction for another molecule. The attractions between molecules are called intermolecular
forces and these are weak forces. Covalent substances have low melting points and boiling points compared to ionic
compounds or metals. At room temperature, covalent substances are gases, liquids or low melting point solids. They do
not conduct electricity as solids or when molten and usually do not conduct when dissolved in water.
Broughton High School
Broughton High School
Broughton High School
Broughton High School of Wake County
Student Workbook Physical Science – Chemical Bonding Mr. Davis
Broughton High School of Wake County
Student Workbook Physical Science – Chemical Bonding Mr. Davis
Broughton High School of Wake County
Student Workbook Physical Science – Chemical Bonding Mr. Davis
Broughton High School of Wake County
Student Workbook Physical Science – Chemical Bonding Mr. Davis