Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

CCEA AS Chemistry Units 1, 2 And 3 > (U1) Atomic Structure > Flashcards

(U1) Atomic Structure Flashcards

(39 cards)

Start Studying
1
Q

What is atomic number?

A

The number of protons in the nucleus of an atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is mass number?

A

The total number of protons and neutrons in the nucleus of an atom.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is Relative Atomic Mass (RAM) (3)

A
  • The weighted mean mass
  • of an atom of an element
  • relative to 1/12 of the mass of an atom of carbon-12
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is Relative Isotopic Mass (RIM) (3)

A
  • The weighted mean mass
  • of an atom of an isotope of an element
  • relative to 1/12 of the mass of an atom of carbon-12
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What are isotopes? (2)

A
  • Atoms which contain the same number of protons
  • but a different number of neutrons
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is Relative Molecular Mass (RMM) (3)

A
  • The weighted mean mass
  • of a molecule
  • relative to 1/12 the mass of an atom of carbon-12
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What is Relative Formula Mass (RFM) (2)

A
  • The weighted mean mass of a species
  • relative to 1/12 the mass of an atom of carbon-12
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is a molecular ion?

A

2 or more atoms covalently bonded with an overall charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is First Ionisation Energy? (2)

A
  • The energy required to convert one mole of gaseous atoms
  • into gaseous ions with a single positive charge
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is Second Ionisation Energy? (2)

A
  • The energy required to convert one mole of gaseous ions with a single positive charge
  • into gaseous ions with a double positive charge
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is Third Ionisation Energy? (2)

A
  • The energy required to convert one mole of gaseous ions with a double positive charge
  • into gaseous ions with a triple positive charge
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Using a mass spectrometer, how do you calculate relative atomic mass?

A

(percentage abundance) x (mass charge ratio) / 100

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is an orbital? (2)

A
  • a region within an atom that can hold up to 2 electrons
  • within opposite spins
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What shape is an S-type orbital?

A

Spherical

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What shape is a P-type orbital?

A

Dumbbell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

State Hund’s Rule (2)

Study These Flashcards
A
  • where electrons have choice between orbitals of equal energy
  • they will fill the orbitals singly as far as possible
17
Q

State the order of filling for energy levels (up to 9th)

Study These Flashcards
A
  • 1s
  • 2s
  • 2p, 3s
  • 3p, 4s
  • 3d, 4p
18
Q

Why is 4s filled before 3d?

Study These Flashcards
A

4s is closer to the nucleus than 3d

19
Q

In s, p, d, f notation, what do the letters represent?

How many electrons can s, p and d hold?

Study These Flashcards
A
  • Sub shells
  • s holds 2, p holds 6, d holds 10
20
Q

What atom does the electronic configuration 1s2 represent?

What does this mean?

Study These Flashcards
A
  • an atom of helium
  • the 1st ‘s’ sub shell is filled with 2 electrons
21
Q

State the general equation for 1st ionization energy

Study These Flashcards
A

X(g) —> X+(g) + e-

22
Q

State the general equation for 2nd ionization energy

Study These Flashcards
A

X+(g) —> X2+(g) + e-

23
Q

State the general equation for 3rd ionization energy

Study These Flashcards
A

X2+(g) —> X3+(g) + e-

24
Q

Why does ionization energy usually increase across a period? (3)

Study These Flashcards
A
  • increased nuclear charge
  • Decrease in atomic radius
  • same number of shielding electrons
25
What is the **electronic configuration** of **Cr** (using *noble gas notation*) **Why** is it **irregular**?
- [Ar] 3d5 4s1 - the **4s subshell** *loses an electron* to the **3d subshell** to form a **half filled subshell** (*more stable*)
26
What is the **electronic configuration** of **Cu** (using *noble gas notation*) **Why** is it **irregular**?
- [Ar] 3d10 4s1 - the **4s subshell** *loses an electron* to the **3d subshell** to form a **filled subshell** (*stable*)
27
What **2 elements** are **exceptions** to the **rule** for the **filling of orbitals**?
- Cu - Cr
28
**Why** does **ionization energy** *not increase regularly* **across a period**?
- some have **higher than expected** energies due to **filled and half filled** subshells - *transition metals* **increase marginally** due to **3d subshell shielding** 4s effectively
29
What happens to *1st ionization energy* **down a group**? **Why**?
- decreases - increase in **atomic radius** and **more energy levels** —> **more shielding** —> **attraction weakens**
30
What are **valence** electrons?
Outer electrons
31
How many **orbitals** are in a: - p-subshell - s-subshell - d-subshell
- p = 3 orbitals - s = 1 orbital - d = 5 orbitals
32
State and explain the **general trend** in the **first ionization energy** *across* the **second period**. Identify and *explain* any **exceptions** (**7**)
- 1st ionization energy **increases left to right** - due to: 1. **increase** in *nuclear* **charge** 2. **Decrease** in **distance** between *nucleus* and *outer electrons* 3. **Same number** of **shielding electrons** - *exceptions*: **Be** and **N** - **Be** —> **full outer subshell** —> *stability* —> *more energy needed* - **N** —> **half full outer subshell** —> *stability* —> *more energy needed*
33
When *forming cations*, which **orbital** are *electrons removed from* first in **Cr**? **Why**?
- The **4s** subshell - 4s has lower energy than 3d
34
What are the **relative masses** and **charges** of: 1. Protons 2. Neutrons 3. Electrons
1. Protons - mass = 1 - charge = +1 2. Neutrons - mass = 1 - charge = 0 3. Electrons - mass = 1/1840 - charge = -1
35
How do you calculate **relative atomic mass** from **mass spectra**? | (equation)
RAM = percentage abundance (%) x mass charge ratio (Z) / 100
36
On the periodic table, where is the: - s-block - p-block - d-block - f-block **Why** are they *called this*?
1. S-block = groups 1 and 2 2. P-block = groups 3 to 8 3. D-block = transition metals 4. F-block = lanthanum series ## footnote Name comes from their **outermost subshell**
37
In **box notation**, how do you *represent electrons*?
**⥮** one arrow up, one arrow down - representing 2 electrons in opposite spins (within an orbital) **⥮**
38
What does a **large difference** (compared to 3rd ionisation energy etc.) between **1st and 2nd ionisation energy** *confirm*? Why? (**2**)
The presence of **energy levels**, and that it is a **group 1 element**: - **first electron lost easily** as it is in a *shell furthest from the nucleus (greater atomic radius)* and separated by *greater shielding*, therefore **electrostatic attraction is weakest** - **2nd electron** *closer to nucleus* and requires **more energy** to *overcome stronger electrostatic attraction*
39
What is the **affect** of **ionisation** on *effective nuclear charge*?
Increased ionisation = greater effective nuclear charge | (greater ratio of protons to electrons)

CCEA AS Chemistry Units 1, 2 And 3 (22 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions