Unit 2: Matter

Question 1

What are subatomic particles?

Answer 1

A sub atomic particle is a particle smaller than an atom, such as: protons, neutrons and electrons

Question 2

What is an ion, what are the different types, and how is it different from an atom?

Answer 2

An ion is a charged atom, it can be either a cation (positively charged atom) or anion (negatively charged atom). The only difference is that an ion is charged and an atom is neutral.

Question 3

What is in the nucleus of an atom?

Answer 3

Only protons and neutrons, which is why you can only gain or lose electrons.

Question 4

In relation to their subatomic particles, what makes ions and isotopes different from normal atoms?

Answer 4

In ions the number of electrons changes, in isotopes the number of neutrons changes.

Question 5

What is a cation and what does the word mean in Greek?

Answer 5

A positively charged atom, cation in Greek means going down. (Electrons are going down)

Question 6

What is an anion and what does the word mean in Greek?

Answer 6

An anion is negatively charged atom and it means going up in Greek (Electrons going up)

Question 7

What does atomic number tell us?

Answer 7

Atomic number tells the number of protons, neutrons and electrons in a neutral atom. It also tells us which element the atom is because the atomic number of an element can never change.

Question 8

Does electron bonding mean electrons being taken away, shared or gained?

Answer 8

Shared.

Question 9

What do you need to put around a bohr model of an atom to show that it’s an ion?

Answer 9

Square brackets and put the negative or positive charge outside the top right corner.

Question 10

The uncertainty principle states…

Answer 10

we cannot know both the positions and speed of a particle, such as a photon or electron, with perfect accuracy

Question 11

Frequency is defined as …

Answer 11

The number of complete wave cycles per second.

Question 12

Wavelength definition and measurement

Answer 12

Total distance covered to complete 1 wave from crest to crest or trough to trough

Question 13

Why was the bohr model considered inconsistent with the principles of quantum mechanics?

Answer 13

It assumed fixed orbits for electrons without considering the uncertainty principle.

Question 14

What is the relationship between frequency and wavelengths?

Answer 14

The frequency of the wave is inversely proportional to its wave length. That means waves with a higher frequency have a short wave length, whole waves with low frequency have longer wavelengths.

Question 15

What is the frequency unit called and what is its symbol?

Answer 15

The frequency unit is called hertz (Hz) and the symbol is v.

Question 16

What is the symbol of wavelength and what are its units?

Answer 16

Lambda (λ) and the units can be meters, nanometers (nm), or micrometers (μm)

Question 17

What fundamental concepts did Rutherford’s model fail to include?

Answer 17

It couldn’t explain why atoms are stable (it predicted electrons would crash into the nucleus) and why atoms give off specific colors of light (it didn’t include energy levels for electrons)

Question 18

What is the SI unit?

Answer 18

Is a standard unit from the international system of units.

Question 19

What is a photon?

Answer 19

A photon is a tiny particle of light that carries energy. It has no mass and moves at the speed of light.

Question 20

What do photons have to do with energy levels?

Answer 20

Photons are absorbed or released when electrons move between energy levels in an atom. The energy of a photon matches the energy difference between the levels, which is why electrons emit or absorb light at specific colors.

Question 21

Wavelength vs Wave cycle vs Wave

Answer 21

Wavelength is a measurement.
Wave cycle is one full repeat of the wave pattern.
Wave is the entire phenomenon itself.

Question 22

How many electrons can s orbital hold?

Answer 22

It can hold 2 electrons.

Question 23

How many electrons can p hold?

Answer 23

It can hold 6 electrons.

Question 24

How many electrons can d orbital hold?

Answer 24

d orbital can hold 10 electrons.

Question 25

How many electrons can f orbital hold?

Answer 25

f orbital can hold 14 electrons.

Question 26

What does the parts of the electron configuration notation nl^x represent?

Answer 26

n = principle quantum number (energy level or shell)
l = subshell (s, b, d, or f indicating orbital shape)
x = number of electrons in the subshell

Question 27

What are isoelectronic species?

Answer 27

Isoelectronic species have similar electron configurations

Question 28

How do you use noble gas configuration

Answer 28

You have to use the last noble gas from the period above and put it in brackets

Question 29

What is the Aufbau principle

Answer 29

Electrons occupy the lowest energy orbital first, then move to the next one and so on

Question 30

Orbitals are considered to be in the same shell if they have the same ___ number

Answer 30

First number (quantum number n)