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3 years ago

Why would two (2) chlorine atoms be stably bonded together?

Chemistry

2 answers:

I am Lyosha [343]3 years ago

7 0

Answer:

Covalent Bonds

Explanation:

The two chlorine atoms are said to be joined by a covalent bond. The reason that the two chlorine atoms stick together is that the shared pair of electrons is attracted to the nucleus of both chlorine atoms. Hydrogen atoms only need two electrons in their outer level to reach the noble gas structure of helium.

A covalent bond, also called a molecular bond, is a chemical bond that involves the sharing of electron pairs between atoms. These electron pairs are known as shared pairs or bonding pairs, and the stable balance of attractive and repulsive forces between atoms, when they share electrons, is known as covalent bonding.

Don't worry I am taking Introduction to Biological Chemistry at the college so I am sure!

Hope this helps!

Over [174]3 years ago

6 0

Answer:

The two chlorine atoms are said to be joined by a covalent bond.

Explanation:

The reason that the two chlorine atoms stick together is that the shared pair of electrons is attracted to the nucleus of both chlorine atoms. Hydrogen atoms only need two electrons in their outer level to reach the noble gas structure of helium.

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How many sulfur atoms are generated when 9.42 moles of H2S react according to the following equation: 2H2S+SO2→3S+2H2O

8_murik_8 [283]

Answer:

A) 8.51 × 10²⁴

Explanation:

1. Gather all the information

2H₂S + SO₂ ⟶ 3S + 2H₂O

n/mol: 9.42

2. Calculate the moles of S atoms

The molar ratio is 3 mol S:2 mol H₂S

$\text{Moles of S} = \text{9.42 mol H$_{2}$S} \times \dfrac{\text{3 mol S }}{\text{2 mol H$_{2}$S }} = \text{14.13 mol S}$

3. Calculate the atoms of S

$\text{Atoms of S } = \text{14.13 mol S} \times \dfrac{6.022 \times 10^{23}\text{ S atoms}}{\text{1 mol S}} = \mathbf{8.51 \times 10^{24}}\textbf{ S atoms}$

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3 years ago

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80cm^3 of oxygen gas diffused through a porous hole in 50 seconds how long wiil it take 120cm^3 of nitrogen (iv) oxide to diffus

inysia [295]

Answer: it will take 89.93secs

Explanation:Please see attachment for explanation

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3 years ago

How to do lewis dot structure of nh3conh3

wlad13 [49]

Answer:

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3 years ago

Write the balanced chemical equation between H2SO4 and KOH in aqueous solution. This is called a neutralization reaction and wil

emmainna [20.7K]

Answer:

0.166M

Explanation:

In a neutralization, the acid, H₂SO₄, reacts with a base, KOH, to produce a salt, K₂SO₄ and water. The reaction is:

H₂SO₄ + 2KOH → K₂SO₄ + 2H₂O

To solve this problem, we need to determine moles of H2SO4 and moles of KOH that reacts to find the moles of sulfuric acid that remains after the reaction:

Moles H2SO4:

0.650L * (0.430mol /L) = 0.2795moles H2SO4

Moles KOH:

0.600L * (0.240mol / L) = 0.144 moles KOH

Moles of sulfuric acid that reacts with 0.144 moles of KOH are:

0.144 moles KOH * (1mol H2SO4 / 2 mol KOH) = 0.072 moles of H2SO4 react.

And remain:

0.2795moles H2SO4 - 0.072moles H2SO4 = 0.2075 moles of H2SO4 reamains.

In 0.650L + 0.600L = 1.25L:

Molar concentration of sulfuric acid:

0.2075 moles of H2SO4 / 1.25L =

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3 years ago

Naphthalene, C10H8, melts at 80.2Â°C. If the vapour pressure of the liquid is 1.3 kPa at 85.8Â°C and 5.3 kPa at 119.3Â°C, use th

sweet-ann [11.9K]

(a) One form of the Clausius-Clapeyron equation is

ln(P₂/P₁) = (ΔHv/R) * (1/T₁ - 1/T₂); where in this case:

P₁ = 1.3 kPa

P₂ = 5.3 kPa

T₁ = 85.8°C = 358.96 K

T₂ = 119.3°C = 392.46 K

Solving for ΔHv:

ΔHv = R * ln(P₂/P₁) / (1/T₁ - 1/T₂)

ΔHv = 8.31 J/molK * ln(5.3/1.3) / (1/358.96 - 1/392.46)

ΔHv = 49111.12 J/molK

(b) Normal boiling point means that P = 1 atm = 101.325 kPa. We use the same formula, using the same values for P₁ and T₁, and replacing P₂ with atmosferic pressure, solving for T₂:

ln(P₂/P₁) = (ΔHv/R) * (1/T₁ - 1/T₂)

1/T₂ = 1/T₁ - [ ln(P₂/P₁) / (ΔHv/R) ]

1/T₂ = 1/358.96 K - [ ln(101.325/1.3) / (49111.12/8.31) ]

1/T₂ = 2.049 * 10⁻³ K⁻¹

T₂ = 488.1 K = 214.94 °C

(c) The enthalpy of vaporization was calculated in part (a), and it does not vary depending on temperature, meaning that at the boiling point the enthalpy of vaporization ΔHv is still 49111.12 J/molK.

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4 years ago