Principles of Science Bonding Basics - Ionic Bonds  

  Complete the chart for each element.  

Element  # of Protons  # of Electrons  # of Valence Electrons 

Charge (Oxidation #) 

Sodium         

Chlorine         

Beryllium         

Fluorine         

Lithium         

Oxygen         

Phosphorus         

 Follow the examples from class to complete each ionic bond. 

 (1) Potassium + Fluorine 

              (2) Magnesium + Iodine 

    

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(3) Sodium + Oxygen             (4) Sodium + Chlorine 

           (5) Calcium + Chlorine 

           (6) Aluminum + Chlorine 

          

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Principles of Science Bonding Basics - Covalent Bonds  Complete the chart for each element.  

Element  # of Protons  # of Electrons  # of Valence Electrons 

# of Electrons to Fill Outer Shell 

Carbon         

Chlorine         

Hydrogen         

Phosphorus         

Oxygen         

Sulfur         

Nitrogen         

 Follow the examples from class to complete each covalent bond. 

 (1) Hydrogen + Hydrogen (H2) 

              (2) Hydrogen + Oxygen (H2O) 

    

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(3) Chlorine + Chlorine (Cl2)              (4) Oxygen + Oxygen (O2) 

           (5) Carbon + Oxygen (CO2) 

            (6) Carbon + Hydrogen (CH4) 

       

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Principles of Science Stability in Bonding / Types of Bonds

Directions: In the blanks, write the terms from the word list that complete the definition. Words can be used more than once.

positive element(s) compound(s) energy level(s) charged number(s) force(s) atom(s) ion(s) electron(s) negative

1. A chemical formula tells what _____________________make up a ____________________ and the

exact __________________ of atoms of each element in a unit of compound.

2. An atom is chemically stable when its outer ________________ is completely filled with

____________________.

3. A chemical bond is a _____________________ that holds _______________together in a

compound.

4. An __________________ that has lost or gained ___________________is called an ion.

5. An ionic bond is the _________________ of attraction between the opposite charges of the

________________ in an ionic _________________.

6. The attraction that forms between __________________ when they share_______________ is known

as a covalent bond.

7. A polar molecule has a slightly________________ end and a slightly ______________ end.

8. A nonpolar molecule does not have oppositely _________________ ends. Only atoms that are

exactly alike can share their _________________ equally.

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Principles of Science Stability in Bonding Directions: Each statement below contains a pair of terms or phrases in parentheses. Circle the term or phrase that makes each statement true. 1. The properties of a compound are (the same as, different from) the properties of the elements that make

up the compound.

2. Na and Cl are chemical (symbols, formulas).

3. NaCl and NaOH are chemical (symbols, formulas).

4. In the formula H2O, the number 2 is a (subscript, superscript).

5. The number 2 in the formula H2O tells you that each unit of this compound contains two (hydrogen,

oxygen) atoms.

6. If a symbol in a chemical formula does not have a subscript after it, a unit of that compound contains

(no atoms, one atom) of that element.

7. The total number of atoms in Fe2O3 is (two, five, six).

8. There are (three, seven, ten) different elements in H2SO4.

9. An atom is chemically stable if its outer energy level (is filled with, contains no) electrons.

10. For atoms of most noble gases and most other elements, the outer energy level is full when it has (3, 8)

electrons.

11. The noble gases do not readily form compounds because they (are, are not) chemically stable.

12. A chemical bond is a (force, chemical) that holds atoms together in a compound.

13. Chemical bonds form when atoms lose, gain, or (share, multiply) electrons. Directions: Complete the table below by using the formula of each compound to identify the elements that each compound contains and the number of atoms of each of these elements in a unit of the compound. The first formula has been done for you.

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Principles of Science Types of Bonds

Directions: Study the diagram below. Write your answers to the questions in the spaces provided.

1. If atom A loses electrons to atom B, a. how many electrons will atom A lose?

b. how many electrons will atom B gain?

c. what will be the oxidation number of atom A?

d. what will be the oxidation number of atom B?

e. what will be the total charge of the compound formed?

f. what type of bond will form?

2. Explain why an element’s oxidation number is related to the group on the periodic table to which it belongs.

Directions: Complete the table comparing ionic compounds and covalent compounds. Characteristic Ionic Compounds Covalent Compounds

How is it formed

Melting/Boiling points (High/Low)

Usual state at room temp

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Principles of Science Key Terms - Chemical Bonds Directions: Match each term in Column I with its description in Column II. Write the letter of the correct term in the space provided.

Column I ____1. binary compound

____2. chemically stable

____3. nonpolar molecule

____4. ion

____5. ionic bond

____6. polar molecule

____7. oxidation number

____8. chemical formula

____9. covalent bond

____10. hydrate

____11. chemical bond

____12. polyatomic ion

Column II a. number that indicates how many

electrons an atom must gain, lose, or share to become stable

b. shorthand that tells what elements a compound contains and the exact number of atoms of each element in a unit of the compound

c. positively or negatively charged, covalently bonded group of atoms

d. compound composed of two elements

e. describes an atom that has a full outermost energy level

f. molecule that has a slightly positive end and a slightly negative end

g. the attraction that forms between atoms when they share electrons

h. the force that holds atoms together in a compound

i. a compound that has water chemically attached to it

j. the force of attraction between the opposite charges of the ions in an ionic compound

k. molecule made of two identical atoms that share the electrons equally

l. a charged particle that has either more or fewer electrons than protons

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Principles of Science Review: Chemical Bonds Directions: All of the statements below are false as written. In the space provided, write a term or phrase that makes the statement true when it is substituted for the underlined words. _________________1. The properties of a compound are the same as the properties of

the elements that it contains.

_________________2. Superscript numbers in chemical formulas tell how many atoms of each element are found in a unit of compound.

_________________3. All the noble gases except helium have 18 electrons in their outer energy level.

_________________4. A(n) chemical formula is the force that holds atoms together in a compound.

_________________5. An ion is a(n) neutral particle that has either more or fewer electrons than protons.

_________________6. Oxidation numbers are written as subscripts.

_________________7. A(n) covalent bond is the force of attraction between the opposite charges of the ions in an ionic compound.

_________________8. The charge on a compound is always positive.

_________________9. Equal sharing of electrons in covalent bonds results in polar molecules.

_________________10. Only two identical atoms can share electrons unequally.

_________________11. A binary compound contains five different elements.

_________________12. An oxidation number tells how many protons an atom must gain, lose, or share to become stable.

_________________13. The oxidation number of the copper(II) ion is 3+.

_________________14. When writing chemical formulas, add superscripts so that the sum of the oxidation numbers equals ten.

_________________15. A polyatomic ion never has a positive or negative charge.

_________________16. The polyatomic ion SO4 is called the sulfide ion.

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Principles of Science Elements and Bonding Worksheet

1) Classify each of the following elements as an alkali metal, an alkaline- earth metal, transition metal, metalloid, halogen, or noble gas based on its position in the periodic table:

• boron __________________________

• gold __________________________

• krypton __________________________

• calcium __________________________

2) How many valence electrons do each of the following elements have?

• carbon ______

• selenium ______

• xenon ______

• potassium ______

3) Which of the following ions are likely to be formed?

● N+5 ______

● He+1______

● F-1 ______

● Al+2 ______

● P-3 ______

● Mg+2 ______

4) Explain why oxygen is a fairly reactive element while neon is not.

5) Explain why beryllium loses electrons when forming ionic bonds, while sulfur gains electrons.

6) Explain why fluorine and chlorine have similar reactivities (the word “valence” should be somewhere in your answer!)

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Principles of Science Review on Bonding

1) Explain why atoms of the noble gases do not easily form bonds, unlike other atoms.

2) State the octet rule and explain how it relates to the formation of a bond.

3) What happens to the stability of an atom when it forms a chemical bond?

4) How does a covalent bond differ from an ionic bond?

5) What are cations and how are they formed?

6) What are anions and how are they formed?

7) Give the charges for ions formed from elements from the following groups. a. Group 1 b. Group 2 c. Group 16 d. Group 17

8) Under the right conditions, ionic substances can conduct electricity very well. Describe these

conditions, and explain why an ionic substance would be a poor choice as a conductor for a computer circuit board.

9) Why do ionic compounds ordinarily have such high melting and boiling points?

10) Using the formula of a compound, how might we determine whether or not it’s ionic?

11) Your lab partner believes that all ions are stable. How would you explain what is wrong with his belief?

12) A classmate insists that sodium gains a positive charge when it becomes an ion because it gains a

proton. Explain this student’s error.

13) Describe the attractive and repulsive forces that occur as two atoms are brought closer together.

14) List three differences between covalent and ionic compounds.

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15) Compare the behavior of bonding electrons in a nonpolar covalent bond with that of bonding electrons in a polar covalent bond.

16) Why is the melting and boiling temperature of a molecular compound usually lower than those of an ionic compound?

17) What are the physical properties of ionic compounds?

18) What are the physical properties of covalent compounds?

19) What is a valence electron?

20) What determines the chemical properties of an element?

21) What is an electron-dot diagram?

22) How are electrons placed in an electron dot diagram?

23) Draw an electron-dot diagram for one element in Groups 1, 2, 13, 14, 15, 16, 17, and 18.

24) Why are most ionic compounds solids at room temperature while covalent compounds are usually gasses or liquids?

25) In an ionic compound, what is total sum of the charges from the cation and the anion?

26) Using electron-dot diagrams, explain the bonding between Aluminum and Chlorine.

27) Using electron-dot diagrams, explain the bonding between Sulfur and Oxygen (SO2).

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