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3 years ago

Give the electron configurations for the elements given. use the noble gas core preceding for the inner electrons.

1 answer:

6 0

Noble Gas Cores have following electronic configuration

He = 1s²
Ne = [He] 2s², 2p⁶
Ar = [Ne] 3s², 3p⁶
Kr = [Ar] 4s², 4p⁶
Xe = [Kr] 5s², 5p⁶

Now solving for question elements,

Germanium = Ge = [Ar] 3d¹⁰, 4s², 4p²

Nickle = Ni = [Ar] 3d¹⁰, 4s²

Tunsten = W = [Xe] 4f¹⁴, 5d⁴, 6s²

Titanium = Ti = [Ar] 3d², 4s²

Iron = Fe = [Ar] 3d⁶, 4s²

Zinc = Zn = [Ar] 3d¹⁰, 4s²

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A sample of ethanol (C2H6O) has a mass of 0.2301 g. Complete combustion of this sample causes the temperature of a bomb calorime

Keith_Richards [23]

Answer: $4.994\times 10^{-3}$ moles

Explanation:

According to avogadro's law, 1 mole of every substance weighs equal to molecular mass , occupies 22.4 L at STP and contains avogadro's number $6.023\times 10^{23}$ of particles.

To calculate the moles, we use the equation:

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

Given mass of ethanol = 0.2301

Molar mass of ethanol = 46.07 g/mol

$\text{Number of moles of ethanol}=\frac{0.2301g}{46.07g/mol}=4.994\times 10^{-3}$

Thus there are $4.994\times 10^{-3}$ moles of ethanol are present in the sample.

7 0

4 years ago

Read 2 more answers

5. Given 18.5 grams of CHA and 24.0 grams of Oz the following reaction occurs. Calculate the number of grams of

ehidna [41]

Answer:

16.5 g of CO₂ are produced by 18.5 of methane and 24 g of O₂

Explanation:

This is a reaction of combustion:

CH₄ + 2O₂ → CO₂ + 2H₂O

1 mol of methane react to 2 moles of oxygen in order to produce 1 mol of carbon dioxide and 2 moles of water.

First of all, we determine the moles of each reactant:

18.5 g . 1mol/ 16g = 1.15 moles of methane

24 g . 1mol / 32g = 0.75 moles of oxygen

Now, we determine the limiting reactant:

1 mol of methane reacts to 2 moles of oyxgen

1.15 moles of methane may react to (1.15 . 2) /1 = 2.3 moles.

We only have 0.75 moles of O₂ and we need 2.3, that's why the oxygen is the limiting reagent, because we do not have enough oxygen for the reaction.

2 moles of O₂ produce 1 mol of CO₂

Then 0.75 moles may produce (0.75 . 1) /2 = 0.375 moles of CO₂

We convert the moles to mass → 0.375 mol . 44g /mol = 16.5 g

7 0

3 years ago

14. In the lab, an experimenter mixes 75.0 g of water (initially at 30oC) with 83.8 g of a solid metal (initially at 600oC). At

avanturin [10]

Answer:

Tungsten is used for this experiment

Explanation:

This is a Thermal - equilibrium situation. we can use the equation.

Loss of Heat of the Metal = Gain of Heat by the Water

$-Q_{m}=+Q_{w}\\$

Q = mΔT $C_{p}$

Q = heat

m = mass

ΔT = T₂ - T₁

T₂ = final temperature

T₁ = Initial temperature

Cp = Specific heat capacity

<u>Metal</u>

m = 83.8 g

T₂ = 50⁰C

T₁ = 600⁰C

Cp = $x$

<u>Water</u>

m = 75 g

T₂ = 50⁰C

T₁ = 30⁰C

Cp = 4.184 j.g⁻¹.⁰c⁻¹

$-Q_{m}=+Q_{w}\\$

⇒ - 83.8 x $x$ x (50 - 600) = 75 x 4.184 x (50 - 30)

⇒ $x$ = $\frac{6276}{46090} = 0.13$ j.g⁻¹.⁰c⁻¹

We know specific heat capacity of Tungsten = 0.134 j.g⁻¹.⁰c⁻¹

So metal Tungsten used in this experiment

8 0

4 years ago

To convert liters of CO2 to moles of CO2, what conversion factor would it be?

MArishka [77]

22.4L.

This is because the standard conversion factor for Liters is 22.4 and in the question it explicitly states liters of CO2.

Therefore, in order to convert Liters of CO2 to Moles of CO2, you'd need to use the conversion factor of 22.4.

Hope this helps!

3 0

3 years ago

Can someone please help me with this

aivan3 [116]

Answer:

Explanation:

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4 0

3 years ago