Question

What is the Lewis structure of calcium carbide?

Answer 1

Hint: Lewis structures, also known as Lewis dot formulas, Lewis dot structures, electron dot structures, or Lewis electron dot structures (LEDS), are diagrams that depict the bonding between atoms in a molecule, as well as any lone pairs of electrons that may be present. Any covalently bound molecule, as well as coordination compounds, can be represented by a Lewis structure.

Complete answer:
The sum of the valence electrons on each individual atom equals the total number of electrons represented in a Lewis structure. Lewis structures do not include non-valence electrons. Following these stages, electrons must be put into the structure based on the total amount of accessible electrons.
Single bonds are used to link the atoms initially.
t-2n electrons remain to be put if t is the total number of electrons and n is the number of single bonds. These should be arranged in lone pairs, with one pair of dots representing each pair of electrons accessible.
Lone pairs should be placed on outside atoms (other than hydrogen) until each outer atom has eight electrons in bonding pairs and lone pairs, at which point more lone pairs can be placed on the central atom. Lone pairs should be put on more electronegative atoms first when in doubt.
Atoms (particularly core atoms) may not have an octet of electrons once all lone pairs have been deposited. The atoms must create a double bond in this scenario; a single pair of electrons is transferred between the two atoms to form a second connection. The atom with the lone pair still has an octet since the bonding pair is shared between the two atoms; the other atom now has two extra electrons in its valence shell.
 $Ca{C}_2$ is the chemical formula for pure Calcium Carbide, which is a white and odourless solid.
Commercial Calcium Carbide, on the other hand, can come in a variety of colours, depending on the impurities present (usually calcium, magnesium, and other oxides).
Calcium Carbide ( $Ca{C}_2$ ) is a chemical compound with the molecular name $Ca{C}_2$ . Calcium acetylide, phenyl glyceryl ether diacetate, and glycerol phenyl ether diacetate are some of the other names for it. At room temperature, calcium carbide appears as a colourless crystalline solid with a rock-like structure.
Each carbon atom has five valence electrons: three from the double bond and two from the lone pair. This results in 7 electrons per carbon nucleus, given the two inner shell electrons. Since each carbon atom has a formal negative charge, the carbide ion (I was about to say the acetylide ion, but that's not right) has a formal 2 charge.
Hence $C{a}^{2+}{[:C\equiv C:]}^{2-}$ is the lewis dot structure of calcium carbide.

Note:
The similar approach may be used to draw Lewis structures for polyatomic ions. When counting electrons, negative ions should have more electrons in their Lewis structures than an uncharged molecule; positive ions should have less electrons. When writing an ion's Lewis structure, the complete structure is enclosed in brackets, and the charge is represented as a superscript outside the brackets on the upper right.