2.1 ATOMS & REACTIONS Flashcards
1
Q
Relative mass and charge of protons, neutrons and electrons.
A
2
Q
Define isotope
A
- Atoms of the same element with same proton number, different number of neutrons and different masses
3
Q
Define relative atomic mass , Ar
A
The weighted mean mass of an atom compared to 1/12th the mass of a carbon-12 atom
4
Q
Define relative isotopic mass
A
The mass of an atom of an isotope compared to 1/12th the mass of a carbon-12 atom
5
Q
Relative atomic mass , Ar equation for isotopic mass spectrometry?
A
6
Q
Chromium ion
A
7
Q
Nitrate ion
A
8
Q
Carbonate ion
A
9
Q
Sulfate ion
A
10
Q
Ammonium ion
A
11
Q
Zinc ion
A
12
Q
Silver ion
A
13
Q
Define the term molar mass , Mr
A
- The mass in grams of any substance that equals 1 mole, (e.g 12g of carbon, 16g of oxygen)
- 12g (Mr) of carbon = 1 mole
- 16g (Mr) of oxygen = 1 mole
14
Q
Define the term Avogardos constant
A
- 6.02×10^23
- this is the number of particles in one mole of any substance
- 1 mole of ANYTHING = 6.02×10^23 particles
15
Q
Define the term mole
A
- the amount of any substance that has the same number of particles as 12g of carbon-12 isotope (6.02 x 10^23)
16
Q
Equation for moles, mass, Mr
A
17
Q
Equation for molar gas volume (RTP)
A
18
Q
Define empirical formula
A
- The simplest whole number ratio of atoms in a compound
19
Q
Define molecular formula
A
- The actual whole number ratio of atoms in a compound
20
Q
What is a salt?
A
- Ionic compounds with metal cation/ammonium cations and anions derived from acid
21
Q
Define hydrated crystal
A
- A crystal with water
22
Q
Define anhydrous crystal
A
- A crystal without water
23
Q
Define water of crystalisation
A
- The number of water molecules in ratio to the crystal compound
24
Q
Equation for concentration, volume, moles
A
25
Equation for **concentration, volume, mass**
26
Equation for **ideal gas equation** and their meanings
p = Pressure **(Pa)**
V = Volume **(m^3)**
n = Moles
R = 8.314 (DATA SHEET)
T = Temperature (K) **(°C+273)**
27
Whats mean by a **standard solution**
- Solution with a known concentration
28
Equation for **percentage yeild**
29
Equation for **atom economy**
30
Why is working at **high atom economy** desirable?
- More **cost-efficient** as more desired product is formed in ratio to by-products
31
Define **acid**
- **Proton (H+) donors** that **dissociate/ionise** in solution
- Strong acids **fully dissociate/ionise** in solution to **release H+** ions whereas weak acids only **partially dissociate/ionise** in solution to **release H+** ions
32
State the 4 common acids
- HCl **(strong)**
- HNO3 **(strong)**
- H2SO4 **(strong)**
- CH3COOH (ethanoic acid) **(weak)**
33
Define **alkali**
- **Water soluble bases** that release **OH-** ions in solution (e.g **NaOH, KOH, NH3**)
34
Define **base**
- **Proton (H+) acceptors** that neutralise acids
35
State the general **neutralisation** reaction
36
State the 5 **neutralisation** equations
37
Equation for **percentage uncertainty**
38
State the **oxidation number** for **uncombined elements** (e.g C, Na, O2)
0
39
State the **oxidation number** for **ions** (e.g Na+, Mg2+)
- Their **charge** number
40
State the **oxidation number** for **combined oxygen** (e.g H2O, CaO)
2-
41
State the **oxidation number** for **combined hydrogen** (e.g NH3, H2S)
1+
42
State the **oxidation number** for **combined oxygen in peroxide** (e.g H2O2)
1-
43
State the **oxidation number** for **combined oxygen in flurorides** (e.g O2F2, OF3)
2+
44
State the **oxidation number** for **combined hydrogen in metal hydrides** (e.g LiH)
1-
45
State the **oxidation number** for **combined fluorine** (e.g NaF, CaF2, AlF3)
1-
46
State the **oxidation number** for **roman numeral compounds** (e.g Fe(II)Cl, N(III)O2- )
- The **roman numeral** number
47
Define **oxidation**
- **Loss of electrons** and **increase** in **oxidation number**
48
Define **reduction**
- **Gain of electrons** and **decrease** in **oxidation number**
