Ask question

Ask question

All categories

3 years ago

10

When naming a compound, which of these is written first?

1 answer:

Mnenie [13.5K]3 years ago

6 0

Answer:

cation

Explanation:

<em>Metal </em>

<em> Nonmetal </em>

<em> Anion </em>

<em> Cation</em>

When naming a chemical compound, <u>the cation</u> is written first before anything else.

A typical ionic compound consists of two components - the cation and the anion. While the <u>cation is positively charged in ion</u>, <u>the anion is negatively charged. </u>The cation of a typical ionic compound is named first before the anion and the name often carries that of the element that composes it.

The name of the element that makes up the anion is modified by removing the last few characters ending the name and replacing it with the suffix 'ide'. For example, NaCl is named sodium chloride.

You might be interested in

What prediction is most likely, based on the data?

Reil [10]

Answer:

b

Explanation:

8 0

4 years ago

Read 2 more answers

I’ll give BRAINLIEST please answer this question fast

geniusboy [140]

Answer:

i think its d im not sure

Explanation:

7 0

4 years ago

Determine the number of protons and neutrons for sulfur-34?<br> I need help!

yuradex [85]

16 protons

18 neutrons

6 0

4 years ago

10. What is the number one cause of habitat loss??

mr Goodwill [35]

Answer:

C) Modernization of humans

4 0

3 years ago

Read 2 more answers

It takes 839./kJmol to break a carbon-carbon triple bond. Calculate the maximum wavelength of light for which a carbon-carbon tr

tresset_1 [31]

Answer:

The maximum wavelength of light for which a carbon-carbon triple bond could be broken by absorbing a single photon is 143 nm.

Explanation:

It takes 839 kJ/mol to break a carbon-carbon triple bond.

Energy required to break 1 mole of carbon-carbon triple bond = E = 839 kJ

E = 839 kJ/mol = 839,000 J/mol

Energy required to break 1 carbon-carbon triple bond = E'

$E'=\frac{ 839,000 J/mol}{N_A}=\frac{839,000 J}{6.022\times 10^{23} mol^{-1}}=1.393\times 10^{-18} J$

The energy require to single carbon-carbon triple bond will corresponds to wavelength which is required to break the bond.

$E'=\frac{hc}{\lambda }$ (Using planks equation)

$\lambda =\frac{6.626\times 10^{-34} Js\times 3\times 10^8 m/s}{1.393\times 10^{-18} J}$

$\lambda =1.427\times 10^{-7} m =142.7 nm = 143 nm$

$(1 m = 10^9 nm)$

The maximum wavelength of light for which a carbon-carbon triple bond could be broken by absorbing a single photon is 143 nm.

6 0

4 years ago