Chemical Reaction Questions

Freshman (College 1st year) ・Chemistry ・MLA ・2 Sources

Question 1: Complete and then stability the following acid-base reaction.

NaOH (aq) + HCl (aq) NaCl (aq) + H2O (l)

Question 2: Balance the following equation.

Oxygen + Ammonia Nitrogen gas + Water
3 O2 (g) + 4 NH3 (g) two N2 (g) + 6 H2O (l)

Question 3: Balance the following equation.

Methane + Oxygen Carbon (IV) oxide + Water
CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (l)

Question 4: Using sodium chloride as an example, quickly explain how an ionic bond is formed.


When elements take phase in a reaction, they tend to gain or lose electrons in the bid to turn out to be stable. There are different types of bonds that are formed when the elements take part in a reaction. The main types of bonds include the covalent, ionic and dative bonds. An ionic bond is formed when the metals and non-metals take part in a chemical reaction. This type of bond involves a metal completely transferring its valence electrons to a non-metal (Helmenstine, 2017). The metals have valence electrons in their outermost energy level; therefore, when reacting with non-metals, they donate the delocalized electrons to the non-metals outermost energy shell. Sodium is an alkali metal; thus, it has one valence electron while chlorine has seven valence electrons since it is a halogen. The sodium atom loses one valence electron to obtain an octet state to the chlorine which also obtains an octet state. The elements are usually stable when they have either octet or duplet state in the case of helium (Bettelheim, Brown, Campbell, Farrell, & Torres, 2012).

Use a diagram to illustrate your answer (only the outermost electrons will be shown)

Question 5: Using water and carbon dioxide as examples, briefly explain the difference between a polar covalent bond and a non-polar covalent bond.


A chemical reaction between non-metals constitutes a covalent bond. A water molecule is formed from the reaction between one oxygen atom and two hydrogen atoms while carbon dioxide from two oxygen atoms and one carbon atom. Both water and carbon dioxide have a covalent bond; however, the bonding in water is described as polar covalent. A polar covalent bond is formed from the unequal distribution of the shared electrons. One of the atoms in the molecules pulls electrons closer to itself strongly than the other atom. Therefore, since the electrons generally carry a negative charge, one end of the molecule will attain a slightly negative charge since the electrons are closer to it. On the other hand, the atom which has less strength in pulling the electron becomes partially positive. In the case of carbon dioxide, there is equal sharing of electrons between the atoms (Helmenstine, 2017)

Question 6: Le Chatelier’s Principle states that if a change of condition is applied to a system in equilibrium, the system will alter the equilibrium position in the direction which best reduces the impact of the change of condition. What will happen to this reaction under the following circumstances?

a) We add acetic acid to the mix? 
A forward reaction will be favoured since more acetic acid will react with ethanol to produce more ethyl acetate and water. However, after some time, the system will attain a new equilibrium position (Bettelheim et al., 2012).
b) We add ethyl acetate to the mix?
The backward reaction will be favored as more of the ethyl acetate will react with water to form more of ethanol and acetic acid.


Bettelheim, F., Brown, W., Campbell, M., Farrell, S., & Torres, O. (2012). Introduction to general, organic and biochemistry. Nelson Education.
Helmenstine, A. (2017). What's a Polar Bond in Chemistry? Definition and Examples. ThoughtCo. Retrieved 17 October 2017, from

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