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Iteru [2.4K]
3 years ago
7

Burning magnesium gives us magnesium oxide. This is an example of a _____ reaction. ______ is the common element involved with a

ll chemical reactions of this kind.
Blank 1. Combustion. Decomposition. Replacement. Synthesis.
Blank 2. Carbon. Hydrogen. Magnesium. Oxygen.
Chemistry
2 answers:
Pani-rosa [81]3 years ago
7 0
1 decomposition 2 oxygen
emmainna [20.7K]3 years ago
4 0

Answer:its {Combustion and Oxygen}

Explanation: combustion means to burn something and as we all know you need oxygen for anything to burn or catch fire

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Consider the following three-step reaction pathway.
Alenkinab [10]

Answer:

NO \longrightarrow N_2O_2 \longrightarrow N_2O \longrightarrow N2

Explanation:

The intermediates are the products of all the steps of the reaction pathway, with the exception of the last one. So the intermediates will be:

  • N2O2 from the first step
  • N2O from the second step

The list from reactant to final product:

NO \longrightarrow N_2O_2 \longrightarrow N_2O \longrightarrow N2

<em>Note: the water is considered a by-product, given that is not the product of interest in this steps.</em>

7 0
4 years ago
What is the formula for the stable binary ionic compound formed between Barium and Oxygen?
xeze [42]

Answer: a. BaO

Explanation:

For formation of a neutral ionic compound, the charges on cation and anion must be balanced. The cation is formed by loss of electrons by metals and anions are formed by gain of electrons by non metals.

Here element barium is having an oxidation state of +2 called as Ba^{2+} cation and O^{2-} is an anion with oxidation state of -2. Thus they combine and their oxidation states are exchanged and written in simplest whole number ratios to give neutral BaO

3 0
3 years ago
1. For each of the following, convert the word equation into a formula equation, BUT do not balance! (4 pts each = 12 pts)
daser333 [38]

Answer:

  • 1a) BaClO₃(s) → BaCl₂(g) + O₂(g)

  • 1b) Cl₂(g) + K₃N(s) → N₂(g) + KCl(s)

  • 1c) Na₃N(aq) + Al(BrO₃)₃(aq) → AlN(s) + Na(BrO₃)₃(aq)

  • 2a) Calcium hydroxide and hydrogen gas

  • 2b) Tin(II) silicate and Lead(IV) permanganate

  • 2c) Magnesium oxide and water

  • 2d) No product

  • 2e) Mercury and iodine

  • 2f) Calcium chloride and iodine

  • 2g) Strontium phosphite and cesium nitride

  • 2h) Carbon dioxide, water, and sulfur dioxide

  • 2i) Iron oxide(III) and carbon dioxide

  • 2j) Magnesium acetate and hydrogen gas

  • 2k) Calcium iodide

Explanation:

1. For each of the following, convert the word equation into a formula equation, BUT do not balance!

a) Barium chlorate → Barium chloride + Oxygen

<u>1. Chemical formulas</u>

Barium chlorate:

  • It is a salt: an ionic compound.
  • Barium has oxidation state +2
  • Chlorate is the ion ClO₃⁻
  • Swap the oxidation numbers to write the subscripts: 2 goes to ClO₃ and 1 goes to Ba
  • Chemical formula Ba(ClO₃)₂
  • It is solid: Ba(ClO₃)₂(s)

Barium chloride:

  • It is a salt: an ionic compount
  • Barium has oxidation state +2
  • Chlorine is in oxidation state -1
  • Swap the numbers to write the subscripts: 2 goes to Cl and 1 goes to Ba
  • BaCl₂
  • It is solid BaCl₂(s)

Oxygen:

  • It is a diatomic gas molecule
  • O₂(g)

<u />

<u>2. Write the unbalanced molecular equation:</u>

  • BaClO₃(s) → BaCl₂(s) + O₂(g)

b) Chlorine + Potassium nitride → Nitrogen + Potassium chloride

<u>1. Chemical formulas</u>

Chlorine:

  • It is a diatomic gas molecule
  • Cl₂(g)

Potassum nitride

  • It is a salt
  • Potassium has oxidation state +1
  • Nitrogen is with oxidation state +3
  • Swap the oxidation states
  • K₃N
  • It is solid: K₃N(s)

Nitrogen:

  • It is a diatomic gas
  • N₂(g)

Potassium chloride

  • It is a salt (ionic compound)
  • Potassium has oxidation state +1
  • Chlorine is in oxidation state -1
  • Swap the oxidation numbers
  • KCl
  • It is solid: KCl(s)

<u>2. Write the unbalanced molecular equation</u>

<u />

  • Cl₂(g) + K₃N(s) → N₂(g) + KCl(s)

c) Sodium nitride + Aluminum bromate → Aluminum nitride + Sodium bromate

<u>1. Chemical formulas</u>

Sodium nitride

  • It is a salt (ionic compound)
  • Sodium has oxidation state +1
  • Nitrogen is with oxidation state -3
  • Swap the oxidation numbers
  • Na₃N
  • It is in aqueous solution
  • Na₃N (aq)

Aluminum bromate

  • Salt
  • Aluminum has oxidation state +3
  • Bromate is the ion BrO₃⁻
  • Swap the oxidation states
  • Al(BrO₃)₃ (aq)

Aluminum nitride

  • Both Al and N have oxidation state 3, which simply
  • AlN(s). It is not soluble in water.

Sodium bromate

  • Na(BrO₃)₃ (aq)

<u>2. Write the unbalanced molecular equation</u>

  • Na₃N(aq) + Al(BrO₃)₃(aq) → AlN(s) + Na(BrO₃)₃(aq)

<h2>This is a long answer with more than 5,000 charaters; thus, I have to add the rest of the explanations on a separate file.</h2><h2></h2><h2>The attached file contains the complete answer.</h2>
Download pdf
4 0
4 years ago
Which describes a step in the process of forming an ionic bond?
Ne4ueva [31]

Answer:

a

Explanation:

bruh its A

8 0
3 years ago
Read 2 more answers
Calculate the frequency of the green light emitted by a hydrogen atom with a wavelength of 546 nm.
Alona [7]

Answer: The frequency of the green light emitted by a hydrogen atom with a wavelength of 546 nm is 5.49 \times 10^{14} s^{-1}.

Explanation:

Given: Wavelength = 546 nm (1 nm = 10^{-9} m) = 546 \times 10^{-9} m

The relation between frequency and wavelength is as follows.

\nu = \frac{c}{\lambda}

where,

\nu = frequency

c = speed of light = 3.0 \times 10^{8} m/s

\lambda = wavelength

Substitute the values into above formula as follows.

\nu = \frac{c}{\lambda}\\= \frac{3.0 \times 10^{8} m/s}{546 \times 10^{-9} m}\\= 5.49 \times 10^{14} s^{-1}

Thus, we can conclude that the frequency of the green light emitted by a hydrogen atom with a wavelength of 546 nm is 5.49 \times 10^{14} s^{-1}.

4 0
3 years ago
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