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# Best Homework Help For o2 lewis structure

## Lewis structure

In Lewis dot structures the electrons are represented as solid dots. In molecule, two oxygen atoms share four electrons and form a double bond completing their respective octets. The four bonded electrons are shown in between two O atoms. The rest of the 4 electrons are present on each oxygen atom as lone pairs. ## Lewis structure Sample Questions

Question 1: How many total valence electrons are present in ?

a) 4                             b) 8
c) 12                           d) 8

Explanation: Each oxygen atom has 8 electrons, 6 of which are valence electrons. There are two O atoms in , and therefore 12 valence electrons.

Question 2: What kind of bond is present in molecule?

a) Covalent bond                             b) Ionic bond
c) Co-ordinate bond                         d) None of the above

Explanation: O is a non-metal. Bond formed between two nonmetals is covalent and is formed by sharing of electrons. In Both O atoms share 4 electrons by forming a double bond. Hence, the bond is covalent

Question 3: What do the two lines represent in Lewis structure of ?

a) Three lone pairs                         b) Three electrons
c) Triple bond                                 d) Double bond

Explanation: In the Lewis structure of There is a double bond shown as the two parallel lines between the O atoms. This is a triple bond, with each bond formed by a pair of electrons, one from each O atom.

Question 4: Which of the following statements about lewis structure of is true?

a) There are 8 nonbonding electrons.                         b) There are 2 bonding electrons.
c) There are two lone pairs.                                        d) There are two double bonds.

Answer: Option a) There are 8 nonbonding electrons.

Explanation: Each oxygen atom has 6valence electrons. Out of these 6 , each O atom uses two electrons in bonding with each other and 4 electrons are left on both O atoms. Thus, total of 8 unpaired electrons (four lone pairs) are there in lewis structure of .

Question 5: Oxygen molecule ( ) doesn’t follows the octet rule

a) True                   b) False

Explanation: Each O atom is surrounded by four dots (lone pairs) and two solid lines (double bond), representing another 4 electrons in the double bond. So each O is surrounded by 8 total valence electrons, completing the octet and making it stable.

Question 6: How many bonding electrons are there in ?

a) 2                        b) 3
c) 4                        d) 6

Explanation: An oxygen atom has a total of 8 electrons, out of which there are 6 valence electrons. In a Molecule total electrons are 16 and valence electrons are 12. The two electrons from each oxygen atom are shared with each other forming a double bond between two O atoms, thus total bonding electrons in lewis structure of is 4.

Question 7: How many double bonds are there in lewis structure of a) 0                        b) 1
c) 2                        d) 3

Explanation: In a molecule two O atoms share 4 electrons with each other forming a double covalent bond between them. Each bond is formed by a pair of electrons and thus 4 electrons give rise to a double bond. In lewis structure the double bond is represented by two solid parallel lines between two O atoms.

Question 8: What do the two dots on an atomic symbol represent in a lewis structure?

a) Lone pair                                           b) Single bond
c) Double bond                                      d) An unpaired electron

Explanation: The lone pair of an atom is represented by two solid dots on the  atomic symbol, in a lewis structure.

Question 9: Valence electrons are-

a) Total electrons in an atom                         b) Electrons in outermost shell
c) Noble gases                                              d) Electrons in outermost subshell

Explanation: Valence electrons are electrons present in the outermost shell of an atom, and can participate in the formation of a chemical bond with other atoms.

Question 10: Pick the incorrect statement about lewis structure-

a) There is a double bond present.                                  b) Each oxygen has a lone pair.

c) The nature of bond present is covalent.                       d) Total valence electrons are 12.

Answer: Option b) Each oxygen has a lone pair.

Explanation: Each oxygen atom has 6 valence electrons. Out of these 6 , each O atom uses two electrons in bonding with each other and 4 electrons are left on both O atoms. Thus, total of 8 unpaired electrons (four lone pairs) are there in lewis structure of , with 2 lone pairs each on O atoms.

### What is the correct Lewis structure for o2?

In an oxygen molecule, the two oxygen atoms share a double bond represented by two solid parallel lines between two O atoms. Each bond is formed by a pair of electrons. A double bond means a total of 4 electrons, 2 coming from each oxygen atom. Each oxygen atom is surrounded by 8 electrons and thus has a complete octet and stable state. The four dots on each oxygen atom represent lone pairs of electrons. ### What is the Lewis dot structure for ?

In Lewis dot structures the electrons are represented as solid dots. In molecule, two oxygen atoms share four electrons and form a double bond completing their respective octets. The four bonded electrons are shown in between two O atoms. The rest of the 4 electrons are present on each oxygen atom as lone pairs. ### How many bonding electrons are in the lewis structure of ?

Each oxygen atom has six valence electrons and they tend to complete their octet of electrons by sharing or receiving electrons from other atoms. In a molecule, the two O atoms share 4 electrons by forming a double bond and complete their octets. So, there are 4 bonding electrons in a molecule. 