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Novosadov [1.4K]
1 year ago
7

Explain how to draw the electron-dot diagram for oxygen.

Chemistry
1 answer:
AlexFokin [52]1 year ago
7 0

The electron dot diagram for the oxygen atom shows six electrons around the symbol of the atom.

<h3>What is the electron dot diagram?</h3>

The electron dot diagram is the diagram of atoms of elements showing only the valence electrons present in the atom represented with dots.

The electron dot diagram for the oxygen atom is drawn as follows:

  • The number of valence electrons in oxygen atom is determined; valence electrons = 6
  • The symbol for the oxygen atom is written
  • The valence electrons are shown as dots around the symbol of the element.

In conclusion, the electron dot diagram uses dots around the symbol of an atom to show the valence electrons in the atom.

Learn more about electron dot diagram at: brainly.com/question/5835591

#SPJ1

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What is the mass in grams of 7.5 x 10^15 atoms of nickel, Ni?
statuscvo [17]
<h3>Answer:</h3>

7.3 × 10⁻⁷ g Ni

<h3>General Formulas and Concepts:</h3>

<u>Math</u>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

  1. Brackets
  2. Parenthesis
  3. Exponents
  4. Multiplication
  5. Division
  6. Addition
  7. Subtraction
  • Left to Right

<u>Chemistry</u>

<u>Atomic Structure</u>

  • Reading a Periodic Table
  • Using Dimensional Analysis
  • Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.
<h3>Explanation:</h3>

<u>Step 1: Define</u>

7.5 × 10¹⁵ atoms Ni

<u>Step 2: Identify Conversions</u>

Avogadro's Number

Molar Mass of Ni - 58.69 g/mol

<u>Step 3: Convert</u>

  1. Set up:                              \displaystyle 7.5 \cdot 10^{15} \ atoms \ Ni(\frac{1 \ mol \ Ni}{6.022 \cdot 10^{23} \ atoms \ Ni})(\frac{58.69 \ g \ Ni}{1 \ mol \ Ni})
  2. Multiply:                                                                                                           \displaystyle 7.30945 \cdot 10^{-7} \ g \ Ni

<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 2 sig figs.</em>

7.30945 × 10⁻⁷ g Ni ≈ 7.3 × 10⁻⁷ g Ni

3 0
3 years ago
Define the following IN YOUR OWN HANDWRITING
k0ka [10]

Answer:

A physical property is a characteristic of matter that is not associated with a change in its chemical composition. Familiar examples of physical properties include density, color, hardness, melting and boiling points, and electrical conductivity.

Explanation:

5 0
2 years ago
A sample of a substance was determined and contained 1.0g of mg and 1.75g of o. what is the empirical formula? (10 pts)
Juliette [100K]
<span>Total mass = 2.75g Mass % of Mg = 1.0g x 100/2.75g = 36.36 % Mass % of O = 1.75g x 100/2.75g = 63.64 % Mol of Mg = 36.36/24 = 1.515 Mol of O = 63.64/16 = 3.977 Ratio of Mol of Mg and O in the substance = (1.515 : 3.977) x 2 = 3 : 8 The empirical formula of substance is Mg3O8</span>
7 0
3 years ago
In the laboratory, hydrogen gas is usually made by the following reaction: Zn(s) + 2 HCl(aq) → H2(g) + ZnCl2(aq) How many liters
IrinaK [193]

<u>Answer:</u> The volume of hydrogen gas collected over water is 2.13 L

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Given mass of zinc = 5.566 g

Molar mass of zinc = 65.4 g/mol

Putting values in above equation, we get:

\text{Moles of zinc}=\frac{5.566g}{65.4g/mol}=0.0851mol

For the given chemical reaction:

Zn(s)+2HCl(aq.)\rightarrow H_2(g)+ZnCl_2(aq.)

As, HCl is present in excess. So, it is considered as an excess reagent.

Zinc is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

1 mole of zinc produces 1 mole of hydrogen gas.

So, 0.0851 moles of zinc will produce = \frac{1}[1}\times 0.0851=0.0851mol of hydrogen gas

To calculate the volume of hydrogen gas, we use ideal gas equation, which is:

PV = nRT

where,

P = Pressure of hydrogen gas = Total atmospheric pressure - vapor pressure of water = (752 - 18.65) mmHg = 733.35 mmHg

V = Volume of the hydrogen gas

n = number of moles of gas = 0.0851 moles

R = Gas constant = 62.3637\text{ L.mmHg }mol^{-1}K^{-1}

T = Temperature of hydrogen gas = 21^oC=[21+273]K=294K

Putting values in above equation, we get:

733.35mmHg\times V=0.0851mol\times 62.3637\text{ L.mmHg }mol^{-1}K^{-1}\times 294K\\\\V=\frac{0.0851\times 62.3637\times 294}{733.35}=2.13L

Hence, the volume of hydrogen gas collected over water is 2.13 L

5 0
3 years ago
Calculate the no. of each atoms presents in 10 grams of calcium carbonate.
raketka [301]

Molar Mass of Calcium carbonate:-

\\ \sf\longmapsto CaCO_3

\\ \sf\longmapsto 40u+12u+3(16u)

\\ \sf\longmapsto 52u+48u

\\ \sf\longmapsto 100u

\\ \sf\longmapsto 100g/mol

  • Given Mass=10g

\boxed{\sf No\:of\;moles=\dfrac{Given\:Mass}{Molar\:Mass}}

\\ \sf\longmapsto No\:of\;moles=\dfrac{10}{100}

\\ \sf\longmapsto No\:of\:moles=0.1mol

Now

\boxed{\sf No\:of\:molecules=No\;of\:moles\times Avagadro\: No}

\\ \sf\longmapsto 0.1\times 6.023\times 10^{23}

\\ \sf\longmapsto 6.023\times 10^{22}molecules

8 0
3 years ago
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