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Olin [163]
2 years ago
10

Sec. 5.1: “Simple Ions”

Chemistry
1 answer:
german2 years ago
5 0

The chemical properties of an atom of an element depends on its electronic configuration.

Ions are formed by loss or gain of electrons by atoms.

<h3>What is electronic configuration of an atom?</h3>

Electronic configuration is the arrangement of electrons around the nucleus of an atom.

  • How much an element reacts depends on its electronic configuration.
  • Noble gases are the least reactive elements because their outer energy levels are filled with octet electrons. (except He, which is full with 2)

In most chemical reactions, atoms try to have the electron configurations of the noble gases by either losing or gaining electrons.

Most atoms want to become stable.

<h3>What is the octet rule?</h3><h3 />

Octet rule is a concept of chemical bonding theory that is based on the assumption that atoms tend to have either empty valence shells (energy levels) or full valence shells of eight electrons. “8 is octet”

<h3>What are Alkali metals and Halogens?</h3>

Alkali Metals and Halogens are the most Reactive Elements

  • As members of Group 1, alkali metals have only one electron in their outermost shell.
  • By losing that 1 electron, an alkali metal can get an electron configuration like a noble gas, with eight electrons in its outermost energy level.

1s22s22p63s23p64s1 is the electronic configuration of potassium.

Potassium will lose the 1 electron in the 4th energy level so that its outmost energy level is empty.

Potassium does not gain 7 electrons to become stable instead of losing because the energy associated with losing one electron is less than that needed to gain 7 electrons.

  • As members of Group 7, the halogens have seven electrons in their outermost shell.
  • By gaining one electron, a halogen can get an electron configuration like a noble gas, with eight electrons in its outermost energy level.

1s22s22p63s23p5 is the electronic configuration of chlorine

Chlorine will gain 1 electron to make its outmost energy level full.

After it losing one electron, potassium has the same electron configuration as chlorine does after it gains one electron.

Both are the same as the noble gas argon 1s22s22p63s23p6

  • The atoms of many elements become stable by achieving the electron configuration of a noble gas.
  • The electrons in the outermost energy level are called valence electrons.

<h3>What are valence electrons?</h3>

To find out how many valence electrons an atom has, check the shorthand electronic configuration.

Magnesium, Mg, has the shorthand electron configuration: [Ne] 3s2

The outermost energy level is the 3 energy level.

This means that a magnesium atom has two electrons, both in the 3s

orbital.

The shorthand electron configuration for phosphorus, P, is: [Ne] 3s23p3

The outermost energy level is the 3 energy level.

This means that each phosphorus atom has five valence electrons: 2 in the 3s

orbital, and 3 in the 3p orbital.

<h3>What are ions?</h3>

  • Atoms Gain or Lose electrons to form ions.
  • All atoms are different because they have different numbers of protons and electrons.

For example, a potassium atom has 19 protons and 19 electrons .

After losing 1 electron, potassium still has 19 protons but now only has 18 electrons .

Because the numbers are not the same, there is a net positive charge.

An Ion is an atom, radical, or molecule that has lost or gained one or more electrons and has a positive or negative charge.

<h3>The formation of potassium ion</h3>

Potassium atom forms an ion with a 1+ charge in the following step:

K ---> K+ + e-

<h3>What are Cations and Anions?</h3>

  • Cation: an ion that has a positive charge.

In the case of chlorine, far less energy is required for an atom to gain one

electron rather than lose its seven valence electrons to become stable.

Show how a chlorine atom forms an ion with a 1- charge:

Cl + e- ----> Cl-

  • Anion: an ion that has a negative charge.

Both an atom and its ion have the same number of protons and neutrons so the nuclei are the same.

But, an atom and its ion have different numbers of electrons.

The chemical properties of an atom depend on the number and configuration of its electrons .

So, an atom and its ion have same number atomic number.

Learn more about atoms, ions, and valence electrons at: brainly.com/question/11552489

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Given the following data: Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) ΔH = −23 kJ 3 Fe2O3(s) + CO(g) → 2 Fe3O4(s) + CO2(g) ΔH = −39
nalin [4]

Answer:

ΔH° = -11 kj

Explanation:

Step 1: Data given

1)   Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g)    ΔH = −23 kJ

2)   3 Fe2O3(s) + CO(g) → 2 Fe3O4(s) + CO2(g)   ΔH = −39 kJ

3)   Fe3O4(s) + CO(g) → 3 FeO(s) + CO2(g) ΔH = +18 kJ

Step 2: The balanced equation

FeO + CO → Fe + CO2

Step 3:  Calculate ΔH for the reaction FeO(s) + CO(g) → Fe(s) + CO2(g).

To get this equation, we need to combine the 3 equations

We have to multiply the third equation by 2.

2Fe3O4(s) + 2CO(g) → 6 FeO(s) + 2CO2(g) ΔH = +54 kJ

<u>This equation we add to the second equation</u>

3Fe2O3(s) + CO(g) + 2Fe3O4(s) + 2CO(g) → 2Fe3O4(s) + CO2(g) + 6FeO(s) + 2CO2 (g)

3Fe2O3(s) + 3CO(g) →  3CO2(g) + 6FeO(s)

ΔH°  = 2*18 + (-39) = 36 - 39 =  -3 kJ

<u>This new equation we will divide by 3 </u>

3Fe2O3(s) + 3CO(g) →  3CO2(g) + 6FeO(s)

Fe2O3(s) + CO(g) →  CO2(g) + 2FeO(s)

ΔH°  =-3/3 = -1 kJ

<u>Now we will substract this new equation from the first equation</u>

Fe2O3(s) + 3CO(g) - Fe2O3(s) - CO(g) → 2Fe(s) + 3CO2(g) -2FeO(s) - CO2(g)

2CO(g)  + 2FeO(s)  → 2Fe(s) + 2CO2(g)

ΔH° = -23kJ +1kJ

ΔH° = -22 kj

<u>The next equation we will divide by 2</u>

2CO(g)  + 2FeO(s)  → 2Fe(s) + 2CO2(g)

CO(g)  + FeO(s)  → Fe(s) + CO2(g)

ΔH° = -22kJ /2

ΔH° = -11 kj

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2 years ago
How many molecules are contained in 103.4g of sulfuric acid?
Ierofanga [76]
<h3>Answer:</h3>

1.827 × 10²⁴ molecules H₂S

<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>

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<h3>Explanation:</h3>

<u>Step 1: Define</u>

103.4 g H₂S (Sulfuric Acid)

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

Avogadro's Number

Molar Mass of H - 1.01 g/mol

Molar Mass of S - 32.07 g/mol

Molar Mass of H₂S - 2(1.01) + 32.07 = 34.09 g/mol

<u>Step 3: Convert</u>

  1. Set up:                              \displaystyle 103.4 \ g \ H_2S(\frac{1 \ mol \ H_2S}{34.09 \ g \ H_2S})(\frac{6.022 \cdot 10^{23} \ molecules \ H_2S}{1 \ mol \ H_2S})
  2. Multiply:                                                                                                            \displaystyle 1.82656 \cdot 10^{24} \ molecules \ H_2S

<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 4 sig figs.</em>

1.82656 × 10²⁴ molecules H₂S ≈ 1.827 × 10²⁴ molecules H₂S

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1 CH4 (g) + 2 O2 (g) -----> CO2 (g) + 2H2O(l) ΔH= - 890 kJ
1 mol           2 mol
1)  If ΔH has minus, it means "release". We need only "release" choices.<span>
2) From reaction
1 mol </span>CH4 (g)  "releases"  ΔH= - 890 kJ  - We do not have this choice.

2 mol  O2 (g)   "release" ΔH= - 890 kJ, so
1 mol  O2 (g)   "release" ΔH= - 445 kJ
Correct answer is B.
3 0
3 years ago
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