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Goryan [66]
3 years ago
5

Water, h2o, is a molecule made of oxygen and hydrogen. the bonds that hold water molecules together are due to shared electrons,

and known as __________ bonds.a)covalent)dependent)ionic eliminated)nuclear

Chemistry
2 answers:
Dmitrij [34]3 years ago
8 0
Covalent bonds keep the hydrogen and oxygen atoms together
Jobisdone [24]3 years ago
4 0

Answer:

a) covalent

Explanation:

Atoms tend to gain, lose or share electrons to be more stable. Most atoms follow the octet rule, which states that atoms tend to complete its valence shell (last level of electrons) with 8 electrons. Oxygen follows this rule, but Hydrogen becomes stable when it has 2 electrons in its valence shell. H and O are non-metals, and they tend to share electrons to complete their valence shell.

Oxygen has 6 electrons in its last level, so it needs 2 electrons to complete its octet. Hydrogen has 1 electron so it needs 1 electron to complete its duet.

As a result, 1 atom of oxygen shares electrons with 2 atoms of hydrogen. This can be represented by a Lewis Structure (attached), where electrons are represented as points around each atom. Covalent bonds are formed by the pair of electrons shared between each pair of atoms. Therefore, in the molecule of water there are 2 covalent bonds.

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Please show some work For the reaction: NO(g) + 1/2 O2(g) → NO2(g) ΔH°rxn is -114.14 kJ/mol. Calculate ΔH°f of gaseous nitrogen
uranmaximum [27]

Answer:

148.04 kJ/mol

Explanation:

Let's consider the following thermochemical equation.

NO(g) + 1/2 O₂(g) → NO₂(g)      ΔH°rxn = -114.14 kJ/mol

We can find the standard enthalpy of formation (ΔH°f) of NO(g) using the following expression.

ΔH°rxn = 1 mol × ΔH°f(NO₂(g)) - 1 mol × ΔH°f(NO(g)) - 1/2 mol × ΔH°f(O₂(g))

ΔH°f(NO(g)) = 1 mol × ΔH°f(NO₂(g)) - ΔH°rxn - 1/2 mol × ΔH°f(O₂(g)) / 1 mol

ΔH°f(NO(g)) = 1 mol × 33.90 kJ/mol - (-114.14 kJ) - 1/2 mol × 0 kJ/mol / 1 mol

ΔH°f(NO(g)) = 148.04 kJ/mol

8 0
3 years ago
Bas +<br> PtF2 →<br> BaF2 +<br> Pts<br> Need to balance it
Basile [38]

it is already balanced

REACTANTS

Barium sulfide (BaS) + platinum (Ii) fluoride

PRODUCT

Barium fluoride (BaF2) + Cooperite (PtS)

Hope this answer helps you dear! take care

5 0
2 years ago
As the energy of the molecules increases, the motion of the molecules _______.
Alexus [3.1K]

Answer:

the motion of molecules increases

6 0
3 years ago
True or Flase: dissolving salt in distilled water creates a homogeneous mixture.
chubhunter [2.5K]

Answer:

true

Explanation:

7 0
3 years ago
Read 2 more answers
A sample of a compound is decomposed in the laboratory and produces 330 g carbon, 69.5 g hydrogen, and 220.2 g oxygen. Calculate
Zarrin [17]

Answer: Empirical formula is C_2H_5O

Explanation: We are given the masses of elements present in a sample of compound. To evaluate empirical formula, we will be following some steps.

<u>Step 1 :</u> Converting each of the given masses into their moles by dividing them by Molar masses.

Moles=\frac{\text{Given mass}}{\text{Molar mass}}

Molar mass of Carbon = 12.0 g/mol

Molar mass of Hydrogen = 1.0 g/mol

Molar mass of Oxygen = 16.0 g/mol

Moles of Carbon = \frac{330g}{12g/mol}=27.5moles

Moles of Hydrogen = \frac{69.5g}{1g/mol}=69.5moles

Moles of Oxygen = \frac{220.2g}{16g/mol}=13.76moles

<u>Step 2: </u>Dividing each mole value by the smallest number of moles calculated above and rounding it off to the nearest whole number value

Smallest number of moles = 13.76 moles

\text{Mole ratio of Carbon}=\frac{27.5moles}{13.76moles}=1.99\approx 2

\text{Mole ratio of Hydrogen}=\frac{69.5moles}{13.76moles}=5.05\approx 5

\text{Mole ratio of Oxygen}=\frac{13.76moles}{13.76moles}=1

<u>Step 3:</u> Now, the moles ratio of the elements are represented by the subscripts in the empirical formula

Empirical formula becomes = C_2H_5O

7 0
3 years ago
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