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Chemestry > Topic 1- Key Concepts in chemistry > Flashcards

Topic 1- Key Concepts in chemistry Flashcards

1
Q

What does aqueous mean?

A

Dissolved in water

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2
Q

Learn some simple formulas of some simple compounds and ions- water, carbon dioxide, chlorine, ammonia, hydrogen, oxygen, ammonium, nitrate, sulphate, hydrogen, carbonate

A

answers on Card 5

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3
Q

Name and explain some hazard symbols

A

Answer on CARD 6

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4
Q

Describe the history of the atom

A
  1. First was John Dalton who describes the atoms as solid spheres
  2. Then was J.J Thompson who describes the plum pudding- where the negative electrons where floating in the positive charge
  3. Then was the Rutherford gold experiment- where he fired positively charged alpha particles at a thin sheet of gold. And more particles deflected then expected-this suggests most of the atom is empty space.
  4. Then was the refined Bohr model - which was supported by many experiments.
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5
Q

Name the particle, relative mass and relative charge

A

answer on card 7

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6
Q

Whats the radius of the atoms

A

-10
10 m.

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7
Q

In an atom the number of protons equals to the number of…

A

electrons

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8
Q

What is an ion

A

is an atom or a group of atoms that has lost or gained electrons

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9
Q

Draw and evaluate a nuclear symbol:

A

on card 8

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10
Q

What are isotopes

A

The have the same number of protons but a different number of neutrons . Same atomic number but a different mass number.

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11
Q

What is the relative atomic mass of an element

A

Is the average mass of one atom ,of the element , compared to 1/12 of the mass of one atom of carbon 12.

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12
Q

Calculative relative atomic mass- Boron has two isotopes, boron -10 boron -11 and their relative abundances are 4 and 16 respectively

A

(10X4) + (11X16)=216

216 divide 20 = 10.8

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13
Q

What do groups represent in the periodic table ?

A

The number of electrons on the outer shell

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14
Q

What do the periods represent in the periodic table ?

A

The number of electron shells

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15
Q

What is a stable electronic structure?

A

full outer shell

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16
Q

What are negative ions

A

They are anions that form when atoms gain electrons

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17
Q

What are positive ions

A

They are cations that form when atoms lose electrons

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18
Q

What does it mean when ions names end with -ate

A

Are negative ions containing oxygen and one other element

19
Q

What does it mean when ions name is ending in -ide

A

Are negative ions contain only one element

20
Q

What is ionic bonding?

A

When a metal and a non-metal react , metal losses electrons to form a positive ion and a non-metal gains electrons to form a negative ion (anion). The oppositely charged ions strongly attract each other through electrostatic forces of attraction.

21
Q

How can you show ionic bonding?

A

Through the dot and cross diagram

22
Q

Properties of ionic compound

A
  1. ) High melting and boiling points because of the strong attraction between ions .Large amounts of energy needed to overcome the attraction
  2. )Many dissolve easily in water , so they are able to carry an electric charge.
  3. ) Solid ionic compounds don’t conduct electricity , because ions are fixed in place and can’t move
23
Q

What are the positives and negatives of using using 2D representations

A

+ shows how atoms are connected

-don’t show the shape and size of the substance

24
Q

What are the positives and negatives of dot and cross diagrams

A

+ used for showing how compounds are formed and where the electrons in the bonds come from
- does not show the size of the atoms and ions or how they are arranged

25
Q

What are the positives and negatives of 3D models

A

+ shows arrangement of the ions

- only shows the outer layer of the substance

26
Q

Properties of simple molecular structures

A
  1. Substances containing covalent bonds usually have simple molecular structures
  2. Forces of attraction between these molecules are very weak
  3. To melt a simple molecular structures you have to break the feeble inter molecular forces not the covalent bonds
  4. The bigger the molecules the stronger the intermolecular forces
  5. Molecular compounds don’t conduct electricity
27
Q

What are polymers?

A

Are molecules made up of long chains of covalently bonded carbon atoms.

28
Q

Properties of giant covalent structures .

A
  1. They aren’t soluble in water
  2. They generally don’t conduct electricity (apart from graphite and graphite.
  3. They have very high melting and boiling points.
29
Q

Describe DIAMOND as a giant covalent structure

A
  • is made up of a network of carbon atoms that each form four covalent bonds.
  • has a rigid lattice structure , making it hard , used to strengthen cutting tools
  • does not conduct electricity because there are no free electrons.
30
Q

Describe graphite as a giant covalent structure

A
  • each carbon atom only forms three covalent bonds
  • there aren’t any covalent covalent bonds between the layers- so its soft and slippery -ideal for lubricating
  • has a high melting point
  • has one decolonised electron , so it conducts electricity
31
Q

Describe graphene as a giant covalent structure

A
  • is one layer of graphite
  • a sheet of carbon atoms joined together in hexagons
  • its one atom thick
32
Q

What is a buckmisterfullerene

A

it has a molecular formula C60 forms a hallow sphere

33
Q

What are nano-tubes

A

are also fullerenes, they are like tiny cylinders of graphene so they conduct electricity

34
Q

What is metalic bonding

A

attraction of the delocalized electrons for the positively charged metal ions

35
Q

Physical properties of metals

A
  • has strong electrostatic forces of attraction
  • malleable
  • good conductors of heat and electricity
36
Q

Difference between metals and non-metals

A
  1. they have different chemical properties
  2. Non-metals generally don’t conduct electricity
  3. Non-metals gain electrons to form a full outer shell, metals lose electrons to gain full outer shell
37
Q

Why does the mass of gas seem to increase.

A

If the mass increases its because at least one of the reactants is gas that is found in air , before the reaction the gas is there its floating around in the air but its not contained in the reaction ,so you cant measure it

38
Q

Why does the mass of gas decrease

A

Because one of the products is a gas, so it can escape before measure

39
Q

What is a relative formula mass?

A

is the relative atomic masses off all the atoms in its formula added together

40
Q

What is the empirical formula?

A

tells you the smallest whole number ration of all atoms in the compound

41
Q

What is the Avogadro’s constant?#

A

6.02X10 power23

42
Q

Equation that relates mass and moles

A

mass

moles X Mr

43
Q

Equation for concentration , mass and volume

A

mass

concentration(dm-3) volume (dm3)

44
Q

Practice calculating empirical formulas

A

Chemestry (3 decks)

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