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GCSE chemistry > Topic 1- Atomic structure & the periodic table > Flashcards

Topic 1- Atomic structure & the periodic table Flashcards

1
Q

What is an atom?

A

The smallest part of an element that can exist.

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2
Q

What is an element?

A

An element is a substanve of only one type of atom.

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3
Q

What is a compound?

A

Two or more elements chemically combined in fixed proportions.

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4
Q

Do compounds have the same properties as their constituent elements?

A

No, they have different properties.

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5
Q

What is a mixture?

A

A mixture consists of two or more elements or compounds not chemically combined together.

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6
Q

Does a mixture have the same chemical properties as it’s constituent materials?

A

Yes, it has the same chemical properties.

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7
Q

What are the 5 methods through which mixtures can be seperated? Do they involve chemical reactions?

A

Filtration, crystallisation, simple distillation, fractional distillation and chromatography. They DO NOT involve CHEMICAL REACTIONS!

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8
Q

Describe the plum pudding model.

A

The atom is a ball of positive charge with negative electrons embedded in it.

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9
Q

Describe the Bohr/ Nuclear model. How did it come about?

A

ALPHA PARTICLE EXPERIMENT CONCLUSIONS:
* The mass of the atom was concentrated at the nucleus.
* The nucleus was positively charged.

THE NUCLEAR MODEL:
* Electrons orbit the nucleus at specific distances. The nuclear model came about throough the alpha particle scattering experiment.

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10
Q

What did James Chadwick do?

A

He provided evidence for the existence of neutrons in the nucleus.

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11
Q

State the relative masses and relative charges of the proton, nuetron and electron.

A

RELATIVE MASSES:
* Proton- 1
* Neutron- 1
* Electron- Very small

RELATIVE CHARGES:
* Proton- +1
* Neutron- 0
* Electron- -1

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12
Q

What is the radius of an atom?

A

0.1 nm

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13
Q

What is the radius of the nucleus?

A

1 x 10^-14 of that of an atom.

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14
Q

What do atoms of the same element have nn common?

A

The same number of protons in the nucleus.

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15
Q

What is an isotope?

A
  • Isotopes are atoms of the same element that have a different number of neutrons
  • Isotopes of he same element have the same elctronic structure, so have the same chemical properties.
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16
Q

What are ions?

A

Ions are charged particles. They are formed when an atoms loses/gains electrons.

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17
Q

What are the properties of metals?

A
  • High boiling point
  • Conduct heat & electricity
  • Shiny
  • Malleable
  • High density
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18
Q

What are the properties of non-metals?

A
  • Low boiling/ melting pint
  • Do not conduct heat/ electricity (except graphite)
  • Dull
  • Brittle, not malleable
  • Low density
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19
Q

What is formed when a metal reacts with a non–metal?

A

An ionic compound.

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20
Q

What is formed when a non–metal reacts with a non-metal?

A

A molecular compoound containing covanlently bonded atoms.

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22
Q

What is a solute?

A

A substance that is dissolved in a solvent.

23
Q

What is a solution?

A

A solute dissolved in a solvent.

24
Q

What is miscible/immiscible?

A

Miscible- Substances that mix together
Immiscible- Substances that do noot mix together

25
What does **soluble** mean?
A substance that can be dissolved ina solvent.
26
What are the **collumns** of periodic table called?
Groups
27
What are the **rows** of the periodic table called?
Periods
28
Are **elements** in the **same group similar?**
* They **may** have **similar chemical properties** * As they have the **same amount of outer shell elctrons**
29
What do **elements** in the **same period** have in **common?**
* The **same** number of **energy levels.** * The **same** number of **shells**
30
What were **elements arranged in order of** **before** the discovery of protons, neutrons & electrons?
In order of **atomic weight.**
31
**Why** were s**ome elements** placed in **inappropriate groups?**
If **strict order of atomic weight** was followed.
32
What did **knowledge of isotopes** make it possible to explain?
Why **order based on atomic weight** was **not always correct.**
33
What did **Mendeleev** do?
* Leaving **gaps** for **undiscovered elements.** * He **changed the order** of **some elements** based on **atomic weight**
34
What are a **majority** of **elements?**
Metals
35
What are **elements in group 1** known as?
The **alkali metals.**
36
Sttate the **characteristics of alkali metals.**
* All have **1 electron in outer shell** * All have **low density** * All are **stored under oil** (to prevent reacction with water/oxygen) * All are **soft**
37
How do **group 1 elemnts react with non-metals?**
* They **form ionic compunds** * Which are **soluble white solids** * Which form **colourless solutions** **ALL GROUP 1 ELEMENTS** REACT IN THIS WAY BECAUSE THEY ALL HAVE **1 ELECTRON IN THEIR OUTER SHELL!**
38
How do **group 1 elements react with water?**
They **form hydroxides** which **dissolves** to form **alkaline solutions.** * They fizz * They float * They move around on surface of water * They melt * Potassium only: lilac flame
39
How do group 1 elemnts react with oxygen?
* **Lithium:** Burns with a strong red flame, produces a white solid * **Sodium:** strong orange flame, white solid * **Potassium:** Lilac flame
40
How do group 1 elements react with **chlorine?**
**Lithium:** **White powder** produced **Sodium:** Burns with a **bright yellow flame,** **clouds of whte powder** **Potassium:** Same as sodium but more **vigorous**
41
How does **reactivity change** moving **down group 1?** Why?
**REACTIVITY INCREASES ⬆** * The **atoms** get **larger** * The **distance** between the **nucleus & outer shell electron increases** * The **attraction from the nucleus decreases** * So **electrons** are **more easily lost**
42
State the **characteristics** of **group 7.**
* **7 electrons** in outer shell * **Coloured** vapours * **Diatomic** moleules * Form **ionic salts with metals** * Form **molecular compounds** with **non-metals**
43
State **group 7 elements** and their **states of matter.**
* **Fluorine (F2)**- pale yellow gas 🟡 * **Chlorine (Cl2)**- pale green gas 🟢 * **Bromine (Br2)**- dark brown liquid 🟤 * **Iodine (I2)**- grey solid 🩶
44
What **changes** occur moving **down group 7?**
* **Higher relative molecular mass** * **Higher** m.p and b.p * **Reactivity decreases**- cannot gain an elcetron as easily
45
A **more reactive halogen displaces a less reactive halogen** from an **aqeous solution of it's salt**. **Show** this.
**Cl₂ + 2 NaBr → Br₂ + 2 NaCl** * In this reaction, an **orange** colour of **Br₂** would appear
46
**Why** does a more **reactive halogen** displace a **less reactive halogen** from an **aqeuos solution of it's salt?**
* **Reactivity decreases going down the group** * The **atoms get larger** * **Less attraction** between **nucleus** and **outer shell electron** * The outer shell electron is **more easily lost**
47
Compare group 1 metals & transition metals.
**SIMILARITIES:** * Both conduct heat & electricity * Both are shiny when polished * Both form ionic compounds with nn-metals **DIFFERENCES:** * Transition metals have higher densities & higher melting points than group 1 metals * They are less reactive than group 1 metals * They are harder than group 1 metals
48
Common **characteristics** of **transition metals:**
* **Have ions **with **different charges** * Form **coloured compounds** * Are **useful as catalysts**
49
What is a catalyst?
* A **chemical substance** that **increases the rate of chemical reaction** * It is **not used up** over the course of the reaction
50
State the **colours of flames** observed when **lithium, sodium and potassium burn in oxygen.**
* **Lithium-** Crimson * **Sodium-** Yellow-orange * **Potassium-** Lilac
51
Describe the **properties** of **noble gases.** Describe the **trends going down the group.**
**PROPERTIES:** * Non-metals * Gases * Low boiling point * Unreactive (have a full outer shell) * Do not easily form molecules (full ouer shell) * 8 electrons in outer shell **TRENDS GOING DOWN:** * Atoms have a latger relative atomic mass * So b.p increases

GCSE chemistry (7 decks)

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