Topic 1 Atomic Structure And The Periodic Table Flashcards
1
Q
Compounds contain 2 or more elements chemically combined in…
A
Fixed proportions
2
Q
What is an ion?
A
A charged particle formed when an atom (or group of atoms) loses or gains electrons.
3
Q
What do state symbols show?
A
The physical state of a substance
4
Q
What are the 4 state symbols?
A
Solid = (s)
Liquid = (l)
Gas = (g)
Aqueous solution = (aq)
5
Q
How are aqueous solutions formed?
A
When a substance dissolves in water
6
Q
What is a pure substance?
A
A substance consisting of only one element or one compound
7
Q
What are the 5 physical separation techniques (used to separate mixtures)?
A
- filtration
- crystallisation
- simple distillation
- fractional distillation
- chromatography
8
Q
What does insoluble mean?
A
Unable to dissolve in a particular solvent
9
Q
What is a solution?
A
Mixture formed by a solute and a solvent
10
Q
What is a solvent?
A
The liquid a solute dissolves in to form a solution
11
Q
What is a solute?
A
The dissolved substance in a solution
12
Q
What is filtration used for?
A
To separate an in insoluble solid from a liquid
13
Q
What equipment is needed to carry out filtration?
A
- beaker (containing a mixture of solid and liquid)
- conical flask
- filter paper
- filter funnel
14
Q
What is the name for a liquid that has passed through a filter (in filtration)?
A
Filtrate
15
Q
What is crystallisation used for?
A
To separate a soluble solid from a liquid
16
Q
What does soluble mean?
A
Able to dissolve in a particular solvent
17
Q
What is the process of crystallisation?
A
allowing the solvent to evaporate slowly by gently heating the solution to leave behind solid crystals
18
Q
What are the steps in carrying out crystallisation?
A
- Place solution in evaporating basin over a Bunsen burner/boiling water bath
- Gently heat solution until all solvent has evaporated, leaving solid crystals behind
19
Q
What equipment is needed to carry out crystallisation?
A
- Bunsen burner/boiling water bath (heat)
- evaporating basin
20
Q
What is simple distillation used for?
A
To separate a solvent from a solution
21
Q
What are the 2 stages of simple distillation?
A
- evaporate the liquid into vapour by heating the solution
- condense the vapour back to a liquid by cooling
22
Q
What equipment/apparatus is needed to carry out simple distillation?
A
- flask
- Bunsen burner
- thermometer
- condenser
- beaker
23
Q
What are the steps in carrying out simple distillation?
A
- Heat the solution (in flask) using Bunsen burner until it boils/all the liquid has evaporated and formed vapour
- Vapour rises up glass tube and thermometer reading increases
- Vapour passes through condenser and is cooled back to liquid
- Liquid is collected in beaker
- Left with solid crystals in flask and liquid in beaker
24
Q
How does the condenser work in simple distillation?
A
condenser surrounds glass tube and keeps it cool as cold water continuously runs through condenser
25
What is **fractional distillation used for**?
To **separate** a **mixture** of **different liquids** into **fractions**
26
In **fractional distillation**, what must the **different liquids being separated have**?
Different boiling points
27
What **equipment/apparatus** is needed to **carry out fractional distillation**?
- a **flask** containing a **mixture of different liquids**
- **fractionating column**
- **thermometer**
- **heater**
- **condenser**
- **beakers**
28
What is a **fractionating column**?
**tall column** full of **small glass beads/rods** that is **cooler** at the **top** than at the **bottom**
29
What **examples** of **mixtures** is **fractional distillation useful** for **separating**?
- **Ethanol** and **water**
- **crude oil** into **fractions**
30
What is **paper chromatography used for**?
To **separate mixtures** of **soluble substances**
31
What **equipment** is needed to **carry out paper chromatography**?
- **chromatography paper**
- **pencil line**
- **solvent**
- **ink/dye dots**
32
What is the **paper called** in **paper chromatography**?
The **stationary phase**
33
What is the **solvent called** in **paper chromatography**?
The **mobile phase**
34
What will a **pure substance produce** on a **chromatogram**?
**One spot**
35
What will an **impure substance/mixture produce** on a **chromatogram**?
**Two or more spots**
36
Why is the **starting line** in **paper chromatography drawn** with a **pencil**?
If a **pen was used**, the **pen ink** would **dissolve in the solvent** and **move up the paper**
37
Who **created** the **plum pudding model**?
**JJ Thompson**
38
What **conclusions** were drawn from the **alpha particle scattering experiment**?
- **most of an atom** is **empty space**
- the **mass** of an **atom** is **concentrated at its centre** (nucleus)
- the **nucleus** is **positively charged**
39
What **replaced** the **plum pudding model** after the **alpha particle scattering experiment**?
The **nuclear model**
40
Who **carried out the alpha particle scattering experiment** and **created the nuclear model**?
**Ernest Rutherford**
41
Who **adapted the nuclear model** by **suggesting that electrons orbit the nucleus at specific distances**?
**Niels Bohr**
42
Which **2 other discoveries** about the **atom** were made **after Niels Bohr**?
- the **nucleus contains small positively charged particles - protons**
- the **existence of neutrons** within the **nucleus**
43
Who **provided the evidence** to show the **existence of neutrons**?
**James Chadwick**
44
What is the **relative charge** of a **proton**?
+1
45
What is the **relative charge** of a **neutron**?
0
46
What is the **relative charge** of an **electron**?
-1
47
What is the **radius** of an **atom**?
**0.1 nm** or **1x10-10m**
48
What is the **radius** of a **nucleus**?
**1x10-14m**
49
What is the **relative mass** of a **proton**?
1
50
What is the **relative mass** of a **neutron**?
1
51
What is the **relative mass** of an **electron**?
**Very small**
52
What is the **equation** to **calculate relative atomic mass**?
(**Mass number** of **isotope 1** x **percentage abundance** of **isotope 1**)+(**mass number** of **isotope 2** x **percentage abundance** of **isotope 2**)**/100**
53
How did the **early periodic tables attempt** to **arrange the elements**?
By **atomic weight** (relative atomic mass)
54
Who **developed** the **first modern Periodic-Table**?
**Dmitri Mendeleev**
55
What **type of element reacts** to **form positive ions**?
**Metals**
56
What **type of element reacts** to **form negative ions**?
**non-metals**
57
What is the **atomic number**?
**number** of **protons/electrons** in an **element**
58
What is the **mass number**?
**Total number** of **protons** and **neutrons**
59
How are the **elements** in the **periodic table arranged**?
By **atomic number**
60
What are **isotopes**?
**Atoms** of the **same element** with **different numbers of neutrons**
61
What does the **group number** of an **element represent**?
**Number of electrons** in its **outer shell**
62
What are the **5 properties** of a **typical non metal** (when **solid**)?
- **poor conductivity electricity**
- **poor conductor heat**
- **dull**
- **low density**
- **brittle**
63
What are the **5 properties** of a **typical metal** (when **solid**)?
- **good conductor electricity**
- **good conductor heat**
- **shiny**
- **high density**
- **malleable**
64
What are the **elements** in **group 0 called**?
**Noble gases**
65
Why are the **noble gases unreactive**?
all have a **full outer shell**
66
Why are the **noble gases**, **gases at room temperature**?
All have **low boiling points** **under room temperature**
67
What do the **boiling points** of the **noble gases increase with**?
**Increasing relative atomic mass (going down the group)**
68
What are the **elements** in **group 1 called**?
**Alkali metals**
69
How **many electrons** do **all group 1 elements** have in their **outer shell**?
**1**
70
What does the **reaction** between an **alkali metal** and **oxygen in the air produce**?
**Metal oxides**
71
What are **4 properties** of the **alkali metals**?
- **soft** (can be cut with a knife)
- **relatively low melting points**
- **low densities**
- **reactive**
72
What does the **reaction** between an **alkali metal** and **chlorine produce**?
**Metal chlorides**
73
What does the **reaction** between an **alkali metal** and **water produce**?
**Metal hydroxide and hydrogen** (**compounds** that **dissolve in water** to **produce alkaline solutions**)
74
What happens when a **group 1 element reacts**?
each of its **atoms loses its outer electron** to **form** a **positively charged ion**
75
Why does the **reactivity** of **group 1 elements increase going down the group**?
**Going down group 1:**
- **outer electron** becomes **further from nucleus**
- **attraction** between **nucleus** and **outer electron decreases**
- **outer electron lost more easily**
76
How do **group 1 metals react** with **chlorine** and **water**?
**Vigorously**
77
What are the **3 trends** for **alkali metals** as you **go down group 1**?
- **increasing reactivity**
- **lower melting and boiling points**
- **higher relative atomic mass**
78
What are the **group 7 elements called**?
**The halogens**
79
Why do the **elements** in **group 7 all have similar reactions**?
**All have 7 electrons in outer shell**
80
What do **all group 7 elements form** and **consist of**?
**Molecules** made up of **2 atoms covalently bonded**
81
What are the **3 trends** for the **halogens going down group 7**?
- **decreasing reactivity**
- **higher melting and boiling points**
- **higher relative atomic mass**
82
What do **group 7 elements form** when they **react with other non metal elements**?
**Covalent compounds**
83
What do **group 7 elements form** when they **react with metals**?
**Ionic compounds**
84
Why does the **reactivity** of the **halogens decrease going down the group**?
- **outer shell** is **further from nucleus**
- **harder to gain an electron**
85
How can a **displacement reaction** occur **between 2 halogens**?
**More reactive halogen** can **displace** a **less reactive halogen** from an **aqueous solution** of its **salt**
86
Where are the **transition metals found** on the **periodic table**?
**middle**
87
What are the **6 properties** of **transition metals** that you would expect of a **’typical metal’**?
- **hard**
- **strong**
- **shiny**
- **high density**
- **good conductors**
- **relatively low reactivity**
88
What are the **3 special properties** of **transition metals**?
- **can form ions** with **different charges**
- **form coloured compounds**
- **good catalysts**
