Chapter #2 (Atomic Structure)

Question 1

What are subatomic particles?

Answer 1

The three types of particles that constitute atoms. electron, proton, neutron. Everything we see is made out of just those three things (electron, proton and neutron)

Question 2

What is the relative mass and relative charge of a proton?

Answer 2

Relative mass: 1
Relative charge: +1

Question 3

What is the relative mass and relative charge of a neutron?

Answer 3

Relative mass: 1
Relative charge: 0

Question 4

What is the relative mass and relative charge of a electron?

Answer 4

Relative mass: 1/1836 or 0.0005 or 1/2000
Relative charge: -1

Question 5

What is the relative mass and charge compared to?

Answer 5

We compare it to proton.

Question 6

What are the two numbers shown on a chemical on the periodic table.

Answer 6

The atomic number = Number of protons.

The mass number.

Question 7

How do you know which number is the mass number and which one is the atomic number?

Answer 7

There is a key on the periodic table that explains

Mass number > Atomic number

Question 8

How do you know the number of protons, electrons, neutrons and mass number?

Answer 8

• Number proton = atomic Number
• Electron = The protons
• Number neutron = mass number - atomic number
• Mass number = number protons + number neutrons

Question 9

What is the structure of a atom?

Answer 9

The number of protons and neutrons are in the middle (both together called the nucleus). The electrons are orbiting randomly around the nucleus because they are attracted to the protons (electrostatic force)

Question 10

What is the definition of isotopes?

Answer 10

Atoms of the same element with different numbers of neutrons.

Question 11

What will change if the isotopes of a chemical are different?

Answer 11

The physical properties will change but the chemical properties will stay the same.

Question 12

What is the basic shape of an atom?

Answer 12

A sphere

Question 13

What is the configuration of an atom?

Answer 13

In the middle there is the nucleus (protons and neutrons).
Orbiting around the nucleus are the electrons.

Question 14

Why do atoms not fall into each other since there is so much space with nothing in them?

Answer 14

Because the electrons orbit around the nucleus so fast that it creates a barrier since negatives and negatives repel each other, and electrons are both negatives.

Question 15

Why do electrons orbit around the nucleus?

Answer 15

Because they are attracted to it the positives.

Question 16

What is diffusion?

Answer 16

The random movement of particles that causes them to spread out and mix, with net movement from high to low.

Question 17

What is the process of diffusion? Explain in depth.

Answer 17

1. The particles in the solid dissociate and dissolve in the water (this step only occurs with substances that are solids).
2. BOTH substances are moving around (diffusing)
   Water particles and dissociated solid particles slide over each other and mix. This occurs at the surface of the crystal.
3. The random movement of particles causes them to gradually spread out. They change directions when they collide with other particles.
4. Once “equally” spaced, the particles continue to move randomly, but there is no change in the net movement.

Question 18

What does the rate of diffusion depend on?

Answer 18

The temperature

The size/mass of the particles.

Question 19

What does increasing the temp do to diffusion?

Answer 19

Increasing the temp. increases the rate of diffusion bcs the particles gain energy and move faster. Gases diffuse faster than liquids because there particles move faster.

Question 20

Why does changing the mass of particles affect the rate of diffusion.

Answer 20

Thesmaller the particle, the faster the rate of diffusuion because with a larger particle and a smaller particle, more energy is needed for larger particle to have same speed as smaller particle.

Question 21

What is a key equation for precipitation reaction (meant to show the movement of particles during diffusion). As a word equation and formula.

Answer 21

ammonia + hydrogenchloride -> ammonium chloride
NH3 +HCl -> NH4Cl

Question 22

How do you find the average mass (Ar) with istopes)

Answer 22

istope 1
(abundance x mass /100) + (the same thing with next istope)

Question 23

What are energy levels or shell or orbitals?

Answer 23

the distances from which the electrons are orbiting the nucleus.

Question 24

What is the max. no. of electrons orbiting in each energy level?

Answer 24

1st - max. 2
2nd - max. 8
3rd - max. 8
4th - max. 18
5th - max. 18
6th - max. 32
7th - max. 32

Question 25

What is a cation?

Answer 25

A positive ion.

Question 26

What is an anion?

Answer 26

A negative ion.

Question 27

When are ions formed?

Answer 27

When atoms gain/lose electrons.

Question 28

Why does it take little energy for ions to form?

Answer 28

because electrons are located on the outside of an atom and electrons have a small mass.

Question 29

Can the no. of protons and neutrons change?

Answer 29

For protons it can change, but it requires A LOT of energy, this occurs in nuclear reactions.

For neutrons, it can only varry with isotopes or it requires A LOT of energy as well.

Question 30

What is the symbol for the proton number?

Answer 30

Z

Question 31

What is the symbol for the mass number?

Answer 31

A