Example of covalent compound having three single covalent bond down is electron structure
Answers
Answer:
Explanation:
Single Covalent Bonds
Hydrogen and chlorine coming together is an example of a single covalent bond. Two hydrogen atoms will also come together to form a single covalent bond, as will two chlorine atoms. In these examples, each individual atom has just one unpaired electron to share with the other atom.
Octet rule - Matter always wants to be in the most stable form. For any atom, stability is achieved by following the octet rule, which is to say all atoms (with a few exceptions) want 8 electrons in their outermost electron shell (just like noble gases). The electrons present in the outermost shell of an atom are called valence electrons.
Exceptions to the octet rule include hydrogen (H) and helium (He) that follow the duet rule instead. They are the first two elements of the periodic table and have a single electron shell which accommodates only 2 electrons. Other exceptions include some group 3 elements like boron (B) that contain three valence electrons. Theoretically, boron can accommodate five more electrons according to the octet rule, but boron is a very small atom and five non-metal atoms (like hydrogen) cannot pack around the boron nucleus. Thus, boron commonly forms three bonds,
start text, end text, start subscript, 3, end subscript, with a total of six electrons in the outermost shell. This also results in some anomalous properties for boron compounds because they are kind of “short of electrons”. It should be thus noted that covalent bonding between non-metals can occur to form compounds with less than an octet on each atom.
In general, achieving the octet configuration (i.e. 8 electrons in the outermost shell) is the driving force for chemical bonding between atoms. Take a look at the outer shell configuration (i.e. number of valence electrons) of three atoms – sodium (Na), chlorine (Cl) and neon (Ne):
Nh3 and Ch3 is the answer .Because both have three single covalent bonds