In a metal-oxide-semiconductor (MOS) device, a thin layer of SiO2 (density = 2.20 Mg/m3) is grown on a single crystal chip of silicon. How many Si atoms and how many O atoms are present per square millimeter of the oxide layer? Assume that the layer thickness is 160 nm.

Answer:

3.52×10⁶ atoms of Si and 7.05×10⁶ atoms of O

Explanation:

It is all about unit conversions.

The area of our MOS is 1 mm². So, we know that the thickness is 160 nm. This data can give us the volume. We convert nm to mm.

160 nm . 1×10⁻⁶ mm /1nm = 1.6×10⁻⁴ mm

By the way, now we can determine the volume of MOS, in order to work with density.

1.6×10⁻⁴ mm . 1 mm² = 1.6×10⁻⁴ mm³

But density is mg/m³, so we convert mm³ to m³

1.6×10⁻⁴ mm³ . 1×10⁻⁹ m³/mm³ = 1.6×10⁻¹³ m³

Now, we apply density to determine the mass of MOS

Density = mass /volume → Density . volume = mass

1.6×10⁻¹³ m³ . 2.20mg/m³ = 3.52×10⁻¹³ mg

To make more easier the calculate, we convert mg to g.

3.52×10⁻¹³ mg . 1g /1000mg = 3.52×10⁻¹⁶ g

To count the atoms, we determine molar mass of SiO₂ → 60.08 g/mol

We need to know moles of Si and O₂ in the MOS

Firstly, we determine amount of MOS: 3.52×10⁻¹⁶ g / 60.08 g/mol = 5.86×10⁻¹⁸ moles

1 mol of SiO₂ has 1 mol of Si and 2 mol of O so:

5.86×10⁻¹⁸ mol of SiO₂ may have:

(5.86×10⁻¹⁸ . 1) /1 = 5.86×10⁻¹⁸ moles of Si

(5.86×10⁻¹⁸ .2) /1 =  1.17×10⁻¹⁷ moles of O₂

Let's count the atoms (1 mol of anything contain NA particles)

5.86×10⁻¹⁸ mol of Si . 6.02×10²³ atoms/ mol = 3.52×10⁶ atoms of Si

1.17×10⁻¹⁷ mol of O₂  . 6.02×10²³ atoms/ mol = 7.05×10⁶ atoms of O

The number of Si and O atoms present per mm² of the oxide layer are respectively; 3.52 × 10⁶ atoms of Si and 7.05×10⁶ atoms of O

We are given;

Area of MOS device; A = 1 mm²

Thickness of layer; t = 160 nm = 1.6 × 10⁻⁴ mm

Formula for volume is;

V = Area * thickness

V = 1.6 × 10⁻⁴ mm × 1 mm² = 1.6 × 10⁻⁴ mm³

Converting volume to m³ gives;

V = 1.6 × 10⁻¹³ m³

Now, to get the mass of MOS, we will use the formula;

Mass = Density * volume

we are given density = 2.20mg/m³

Thus;

Mass = 1.6 × 10⁻¹³ m³ × 2.20mg/m³

Mass = 3.52 × 10⁻¹³ mg = 3.52×10⁻¹⁶ g

From periodic table, the molar mass of SiO₂ = 60.08 g/mol

Then;

Number of moles of MOS = (3.52 × 10⁻¹⁶ g)/60.08 g/mol

Number of moles of MOS = 5.86 × 10⁻¹⁸ moles

Now, 1 mol of SiO₂  is formed from 1 mol of Si and 2 mol of O. Thus;

5.86×10⁻¹⁸ mol of SiO₂ will have;

5.86×10⁻¹⁸ moles of Si

and (5.86×10⁻¹⁸ .2) =  11.72 × 10⁻¹⁸ moles of O₂

From Avogadro's number that 1 mol equals 6.02×10²³ atoms , we can say that;

5.86 × 10⁻¹⁸ mol of Si × 6.02 × 10²³ atoms/mol = 3.52 × 10⁶ atoms of Si

11.72 × 10⁻¹⁸ mol of O₂ × 6.02 × 10²³ atoms/mol = 7.05×10⁶ atoms of O

Read more about number of atoms at; https://brainly.com/question/3157958

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