Atomic Structure

Question 1

Atomic Structure: The Atom

What are the Subatomic Particles?

Answer 1

• Protons
• Electrons
• Neutrons

Question 2

Atomic Structure: The Atom

What is the Relative Mass of a Proton?

Answer 2

1

Question 3

Atomic Structure: The Atom

What is the Relative Charge of a Proton?

Answer 3

+1

Question 4

Atomic Structure: The Atom

What is the Relative Mass of an Electron?

Answer 4

0

Question 5

Atomic Structure: The Atom

What is the Relative Charge of an Electron?

Answer 5

-1

Question 6

Atomic Structure: The Atom

What is the Relative Mass of a Neutron?

Answer 6

1

Question 7

Atomic Structure: The Atom

What is the Relative Charge of a Neutron?

Answer 7

0

Question 8

Atomic Structure: The Atom

Which one’s greather Atomic number or Mass number?

Answer 8

Mass number

Question 9

Atomic Structure: The Atom

What is the Atomic Number?

Answer 9

Proton number

Question 10

Atomic Structure: The Atom

What is the Mass Number?

Answer 10

Total number of protons & neutrons

Question 11

Atomic Structure: Isotopes

What is an Isotope?

Answer 11

Atoms with the same atomic number but different mass number

Question 12

Atomic Structure: Isotopes

Which properties do Isotopes share?

Answer 12

Chemical
↳ have the same electron configuration

Question 13

Atomic Structure: Isotopes

Which properties in Isotopes differ?

Answer 13

Physical
↳ depend on its mass

Question 14

Atomic Structure: Relative Mass

What is the Relative Atomic Mass?

Answer 14

Average mass of an atom compared to 1/12 of carbon 12

Question 15

Atomic Structure: Relative Mass

What is the Relative Isotopic Mass?

Answer 15

Average mass of an isotope compared to 1/12 of carbon 12

Question 16

Atomic Structure: Relative Mass

What is meant by the term ‘Abundance’?

Answer 16

How much

Question 17

Atomic Structure: Relative Mass

How would you workout the Ar from Isotopic Abundances?

Answer 17

• Multiply each relative isotopic mass by its % relative isotopic abundance
• Add them up
• Divide by 100

Question 18

Atomic Structure: Mass Spectra

What does the Mass Spectra show?

Answer 18

• Relative Isotopic Masses
• Abundances of diff elements

Question 19

Atomic Structure: Mass Spectra

What does the y-axis show?

Answer 19

The abundance of ions

Often as %

Question 20

Atomic Structure: Mass Spectra

What does the Height of the peak show?

Answer 20

Relative Isotopic Abundance

Question 21

Atomic Structure: Mass Spectra

What does the x-axis show?

Answer 21

m/z or the Relative Isotopic Mass

Question 22

Atomic Structure: Mass Spectra

How would you workout the Relative Atomic Mass from a Mass Spectra graph?

Answer 22

• Multiply each Relative Isotopic Mass by its Relative Isotopic Abundance
• Add them up
• Divide by the sum of Isotopic Abundances

Question 23

Atomic Structure: Mass Spectra

How would you workout the Relative Abundance for Diatomics?

Answer 23

• Express each % as a decimal
• Make a table showing each possible mol
• Add together any duplications

Question 24

Atomic Structure: Mass Spectra

How would you workout the Mass Spectrum for Diatomics?

Answer 24

• Divide all Relative Abundances by the smallest one
  ↳ works out the smallest whole number ratio

Question 25

# **Atomic Structure:** Electron Structure What is meant by the term 'Configuration'?

Answer 25

Arrangement

Question 26

# **Atomic Structure:** Electron Structure What are the 4 Subshells? | (blocks)

Answer 26

* S * P * D * F

Question 27

# **Atomic Structure:** Electron Structure What is an Orbital?

Answer 27

Space where you find electrons

Question 28

# **Atomic Structure:** Electron Structure How many electrons can each orbital hold?

Answer 28

Level 1 (s) = 2 Level 2 (s+p) = 8 Level 3 (s+p+d) = 18 Level 4 (spdf) = 32

Question 29

# **Atomic Structure:** Electron Structure What is S Block Shape?

Answer 29

Spherical

Question 30

# **Atomic Structure:** Electron Structure What is the P Block Shape?

Answer 30

Dumbbell

Question 31

# **Atomic Structure:** Electron Configuration What are its Rules?

Answer 31

1. Electrons enter the lowest available energy level 2. No 2 electrons can have the same spin 3. When in orbitals of equal energy, electrons will try to remain unpaired

Question 32

# **Atomic Structure:** Electron Configuration How would u formulate a Condensed one?

Answer 32

1. Locate element of choice 2. Find **noble gas** that comes DIRECTLY **before** your element 3. Put the **chemical symbol** of that **noble gas** in **squared brackets** 4. Complete the rest of the configuration

Question 33

# **Atomic Structure:** Electron Configuration What's Chronium's EC?

Answer 33

* **Donate one** of their **4s electron** to their **3rd shell** ↳ **more stable** with a **full/half full d-shell**

Question 34

# **Atomic Structure** Electron Configuration What's Copper's EC?

Answer 34

* **Donate one** of their **4s electron** to their **3rd shell** ↳ **more stable** with a **full/half full d-shell**

Question 35

# **Atomic Structure:** Electron Configuration What are Isoelectric Ions?

Answer 35

Different charged ions with the same electron configuration

Question 36

# **Atomic Structure:** Atomic Emission Spectra What happens when an electron is given EMR?

Answer 36

It absorbs the heat ↳ giving it enough energy to jump to a higher QL

Question 37

# **Atomic Structure:** Atomic Emission Spectra What happens to that same electron over time?

Answer 37

It will fall back to its OG QL ↳ releasing heat

Question 38

# **Atomic Structure:** Ionisation Energies What is meant by the term 'Ionisation Energy'? | (endo)

Answer 38

Amount of energy needed to remove electrons from atoms

Question 39

# **Atomic Structure:** Ionisation Energies What is the 1st Ionisation Energy?

Answer 39

Energy required to remove **ONE MOLE** of electrons from **ONE MOLE** of gaseous atoms to form **ONE MOLE** of gaseous positive ions

Question 40

# **Atomic Structure:** Ionisation Energies What are the factors affection Ionisation energy?

Answer 40

* **Atomic Radius** : smaller = greater attraction to nucleus * **Nuclear Charge** : more electrons = greater pull from nucleus * **Shiedling** : less pull from nucleus **:** blocked by inner electrons

Question 41

# **Atomic Structure:** Ionisation Energies What happens to the Ionisation Energy as u go Down a group?

Answer 41

Decreases

Question 42

# **Atomic Structure:** Ionisation Energies Why does the Ionisation Energy decrease going Down a group?

Answer 42

* Down a group, the bigger the Atomic Radius ↳ has more shells * Less Nuclear Charge ↳ easier to remove outer electrons **:** Shielding

Question 43

# **Atomic Structure:** Ionisation Energies What is meant by Successive Ionisation Energy?

Answer 43

As you ionise something successively, you ionise it more than once

Question 44

# **Atomic Structure:** Ionisation Energies Why is the Successive Ionisation Energy higher?

Answer 44

- Positively charged ions have a greater number of protons than electrons ↳ more energy is needed **:** as you're staring from a positive level rather than neutral

Question 45

# **Atomic Structure:** Ionisation Energies What is meant by the term '2nd Ionisation Energy'?

Answer 45

Energy required to remove **ONE MOLE** of electrons from **ONE MOLE** of gaseous ions to form **ONE MOLE** of **TWO** gaseous positive ions

Question 46

# **Atomic Structure:** Ionisation Energies How would u workout an element's group using a table with its data values?

Answer 46

1. Locate the biggest adjacent numeric jump 2. Element's group is based on where the jump starts

Question 47

# **Atomic Structure:** Periodicity What is meant by the term 'Periodicity'?

Answer 47

Trends

Question 48

# **Atomic Structure:** Periodicity What happens to the Atomic Radius across a period? Why? | Size of the atom

Answer 48

**DECREASES** ↳ because the nuclear charge increases & attracts the outer electrons closer to the nucleus

Question 49

# **Atomic Structure:** Periodicity What happens to the Ionisation Energy across a period? Why? | General trend of ionisation across QL 2 & 3

Answer 49

**GENERALLY INCREASES** ↳ proton number increases **:** stronger nuclear charge

Question 50

# **Atomic Structure:** Periodicity Why is there a drop in energy between Mg & Al?

Answer 50

* **Further away** from the **nucleus**, the **more energy** that **electron** has ↳ has less attraction from nucleus * Its **outershell** is **shielded** by the **inner elecrons** ↳ this makes the outershell of electrons to be lost easily * Therefore it is easier to remove that outshell which requires **less heat**

Question 51

# **Atomic Structure:** Periodicity Why is there a drop in energy between P & S?

Answer 51

* Sulfur **refills its 1st orbital** due to its configuration * When **electrons** are **paired** they exert a force of **repulsion** ↳ this force is enough to make the energy drop

Question 52

# **Atomic Structure:** Periodicity What happens to the Mp/Bp across a period? Why? | (For metals)

Answer 52

**INCREASES** * metallic bonds get stronger

Question 53

# **Atomic Structure:** Periodicity What happens to the Mp/Bp across a period? Why? | (For non-metals)

Answer 53

**DECREASES** * LFs are weak & easy to overcome

Question 54

# **Atomic Structure:** Periodicity What happens to Mp/Bp when the Atomic radius increases?

Answer 54

**INCREASES** * there are more electrons **:** more LFs ↳ more energy needed to break bonds