How do lone pairs of electrons affect the bond angle differently than electrons shared in a bond?

Physics

1 answer:

lubasha [3.4K]3 years ago

3 0

Answer:

Lone pairs cause bond angles to deviate away from the ideal bond angles

Explanation:

Bonded electrons are stabilized and clustered between the bonding electrons meaning they are much closer together. Non-bonding electrons however are not being shared between any atoms which allows them to roam a little further spreading the charge density over a larger space and therefore interfering with what would be an expected bond angle

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Calculate the height of a column of carbon tetrachloride, CCl4(l), with a density of 1.59 g/mL that exerts the same pressure as

julia-pushkina [17]

Answer:

1.30 m

Explanation:

The pressure (P) exerted by a column of a liquid can be calculated with the following expression:

$P=\rho \times g \times h$

where,

ρ is the density of the liquid

g is the gravity

h is the height of the column

If both liquids exert the same pressure:

$PHg = PCCl_{4}\\\rho Hg \times g \times hHg = \rho CCl_{4} \times g \times hCCl_{4}\\\rho Hg \times hHg = \rho CCl_{4} \times hCCl_{4}\\hCCl_{4 = \frac{\rho Hg \times hHg}{\rho CCl_{4}} =\frac{13.6g/mL \times 15.2cm}{1.59g/mL} = 130cm=1.30m$