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4 years ago

Is thiamine mononitrate an ionic bond or covalent bond?

Chemistry

2 answers:

MrRa [10]4 years ago

5 0

It is a covalent bond. Whenever a compound uses such suffixes like mono, di, tri, tetra, and so on, it is a covalent compound- thus having covalent bonds.

seropon [69]4 years ago

3 0

Answer:

It's a covalent bond

Explanation:

The diference of electronegativity between the two atoms bonding can help you to decide if a bond is either covalent or ionic.

As shown in the figure, the oxygen atoms of the nitrate (left) will interact with the nitrogen atom of the thiamine(right).

The oxygen have an electronegativity of 3.5 (one of the most electronegative elements) and the nitrogen a 3.0

Being the difference: 3.5 - 3.0=0.5

Now, how this helps to decide the type of bond? For covalent bonds it's expected to have a electronegativity diffetence of < 1.5. On the other hand, for ionic bonds this value should be > 1.5

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What kind of hydrocarbon is this? C-C-C-C-C-C-C-C-OH Please help ASAP

Mice21 [21]

Answer:

1-Octanol

Explanation:

Count the amount of carbon atoms in the chain. Nomenclature includes the position of the largest functional group position in the molecule.

In this case the carbon chain has 8 carbon atoms and one hydroxide functional group (OH)

1 (hydroxide is listed first in the carbon chain) - Oct(8 carbons) + anol (Alkanol hydrocarbon with a hydroxide group, use anol suffix )

= 1 - Octanol

7 0

3 years ago

Hello people ~

son4ous [18]

The m.p. and b.p. of Po, is lower than Te due to

a) inert pair effect

7 0

2 years ago

Is hc2h3o2 quadraprotic?

agasfer [191]

No it isn’t.
do u mean quadratic either way it’s isn’t.
sorry for not much help xox

8 0

3 years ago

If you have access to stock solutions of 1.00 M H3PO4, 1.00 M of HCl, and 1.00 M NaOH solution, (and distilled water of course),

garri49 [273]

Answer:

0.10L of 1.00M of H₃PO₄ and 0.1613L of 1.00M NaOH

Explanation:

The pKa's of phosphoric acid are:

H₃PO₄/H₂PO₄⁻ = 2.1

H₂PO₄⁻/HPO₄²⁻ = 7.2

HPO₄²⁻/PO₄³⁻ = 12.0

To make a buffer with pH 9.40 we need to convert all H₃PO₄ to H₂PO₄⁻ and an amount of H₂PO₄⁻ to HPO₄²⁻

To have a 50mM solution of phosphoures we need:

2L * (0.050mol / L) = 0.10 moles of H₃PO₄

0.10 mol * (1L / mol) = 0.10L of 1.00M of H3PO4

To convert the H₃PO₄ to H₂PO₄⁻ and to HPO₄²⁻ must be added NaOH, thus:

H₃PO₄ + NaOH → H₂PO₄⁻ + H₂O + Na⁺

H₂PO₄⁻ + NaOH → HPO₄²⁻ + H₂O + Na⁺

Using H-H equation we can find the amount of NaOH added:

pH = pKa + log [A⁻] / [HA] (1)

Where [A-] is conjugate base, HPO₄²⁻ and [HA] is weak acid, H₂PO₄⁻

pH = 7.40

pKa = 7.20

[A-] + [HA] = 0.10moles (2)

Replacing (2) in (1):

7.40 = 7.20 + log 0.10mol - [HA] / [HA]

0.2 = log 0.10mol - [HA] / [HA]

1.5849 = 0.10mol - [HA] / [HA]

1.5849 [HA] = 0.10mol - [HA]

2.5849[HA] = 0.10mol

[HA] = 0.0387 moles = H₂PO₄⁻ moles

That means moles of HPO₄²⁻ are 0.10mol - 0.0387moles = 0.0613 moles

The moles of NaOH needed to convert all H₃PO₄ in H₂PO₄⁻ are 0.10 moles

And moles needed to obtain 0.0613 moles of HPO₄²⁻ are 0.0613 moles

Total moles of NaOH are 0.1613moles * (1L / 1mol) = 0.1613L of 1.00M NaOH

Then, you need to dilute both solutions to 2.00L with distilled water.

4 0

3 years ago

Can anybody help me asap pls

Usimov [2.4K]

Answer:

Here is ur answer...

Explanation:

2) Half-filled d orbital increases the stability of the element.

4 0

3 years ago

Read 2 more answers