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Chemistry Flashcards

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1
Q

What is an Isotope?

A

An Isotope is two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei

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2
Q

1.1 Atomic Structure

What is the atomic number?
Where is it located?

A

The atomiv number is the total number of protons
It is located at the bottom of the element

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3
Q

1.1 Atomic Structure

What is the atomic mass?
Where is it located?

A

The atomic mass is the total number of protons and neutrons
The atomic mass is located at the top of the element

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4
Q

1.1 Atomic Structure

How do you calculate the number of neutrons?

A

The number a neutrons is calculated by minusing the stomic number from the atomic mass
Total number of neutrons = Mass - Atomic number

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5
Q

1.1 Atomic Structure

What is an isotope?

A

Isotopes are variations of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei, and hence differ in relative atomic mass but not in chemical properties

(equal atomic number - bottom - and inequal atomi

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6
Q

1.1 Atomic Structure

Calculate the: Atomic number, Proton Number, Mass Numer, Neutron Number, and stablility (stable or unstable) of these elements:

16
O
8

and

18
O
8

A

No 1
Atomic number: 8
Proton Number: 8
Mass Numer: 16
Neutron Number: 8
Stablility: Stable

No 2
Atomic number: 8
Proton Number: 8
Mass Numer: 18
Neutron Number: 10
Stablility: Stable

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7
Q

1.1 Atomic Structure

How can you tell if an atom is stable or unstable?

A

For an atom to be stable they must have a full valence (outer shell) if an atom is unstable if there are too many protons over neutrons or too many neutrons over protons.

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8
Q

1.1 Atomic Structure

What is the Reletive Atomic Mass (RAM)?

A

The reletive Atomic Mass is a weighed average of all the isotopes of an element.

(the numer on the RHS of an element on a periodic table)

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9
Q

1.2 Periodic Table

What do the collums on the periodic table help you to identify?

A

The collums on the periodic table help you to identify the number of electons in the valence shell

skipping 3-12 (lower level on table)

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10
Q

1.2 Periodic Table

What do the rows on the periodic table help you to identify?

A

The rows on the periodic table help you to identify the number of shells each element has

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11
Q

1.2 Periodic Table

What type of element is located on the LHS of the table?

A

Metals are located on the LHS of the periodic table as they have less then 4 electrons iin their valence shell

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12
Q

1.2 Periodic Table

What type of element is located on the RHS of the table?

A

Non - Metals are located on the LHS of the periodic table as they have more then 4 electrons iin their valence shell

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13
Q

1.2 Periodic Table

What does the last collum in the periodic table help you to identify?

A

The last collum in the periodic table hold the most stable elements as they all have 8 elections in the valence shell (full outer shell) meaning they are non-reactive and don’t form chemical reactions

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14
Q

1.3 electronic configuration

How many electrons can fill each orbit shell of an atom?

A

Shell 1 = 2
Shell 2 = 8
Shell 3 = 8
Shell 4 = 2

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15
Q

1.3 electronic configuration

When is a atom most stable?

A

An atom is most stable when it’s valence shell is full

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16
Q

1.3 electronic configuration

What is the electronic configuration of Boron ^5?
What would it do to stabalise itself?

5 = mass no.
11 = atomic no.

A

Electronic configuration = 2.3
Stablise = lose 3 electrons

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17
Q

1.3 electronic configuration

What is the electronic configuration of Carbon ^12?
What would it do to stabalise itself?

6 = atomic no.

12 = mass no.

A

Electronic configuration = 2.4
Stablise = gain 4 electrons

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18
Q

1.4 Formation of Ions

Whats the Octet Rule?

A

Refers to how atoms are most stable when they have 8 electrons on their outermost shell

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19
Q

1.4 Formation of Ions

What is a Cation?

A

A cation is a positively charged ions

pos because they have lost 1 negetive charge (e’) so have more protons

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20
Q

1.4 Formation of Ions

What is an Anion?

A

Anions are negatively charged ions

neg because they have gained 1 negetive charge (e’) so have more e’

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21
Q

1.4 Formation of Ions

What is the new ion form when an element loses electrons?

E.g Na

A

= Na^+

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22
Q

1.4 Formation of Ions

What is the new ion form when an element gains electrons?

E.g Na

A

= Na^-

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23
Q

1.4 Formating

What is subscript?
When is it used?

A

A subscript is a character that is set slightly below the normal line of text.

Subscripts help to convey the composition of molecules, which is essential for understanding chemical formulas and reactions.

  • Chemical Formulas: Subscripts indicate the number of atoms of each element in a molecule. For example, in H₂O, the subscript ‘2’ indicates there are two hydrogen atoms in each water molecule.
24
Q

1.4 Formating

What is super-script?
When is it used?

A

A superscript is a character that is set slightly above the normal line of text.

  • Ions: Superscripts denote the charge of an ion. For example,
    Na^+ indicates a sodium ion with a positive charge, and Cl^- indicates a chloride ion with a negative charge
  • Isotopes: Superscripts are used to indicate the mass number of isotopes. For example, Ca^14 represents carbon-14, an isotope of carbon with 14 nucleons (protons and neutrons).
25
Q

1.5 Ionic Bonding

What is Ionic Bonding?

A

Ionic Bonding is formed between metals and non-metals

Metals lose electrons (cations) non-metals gain electrons (anions)

26
Q

1.5 Ionic Bonding

What is an Ion?

A

An ion is an atom or element with a net electric charge due to the loss or gain of one or more electrons.

27
Q

1.5 Ionic Bonding

What is a Polyatomic Ion?

A

A polyatomic ion is a charged ion composed of two or more atoms covalently bonded together. These ions have an overall charge because the total number of electrons does not equal the total number of protons in the molecule or complex

E.g. NO^-3

28
Q

Whats the difference between an Ion and Polyatomic Ion?

A

An ion can be a single atom or a group of atoms, while a polyatomic ion specifically refers to a group of atoms bonded together with an overall charge.

29
Q

1.6 Ionic Formula

What is the Criss Cross method?

A

The Criss-Cross Method refers to when you switch the charges of each element, to help writing the formula for ionic compounds by ensuring the total positive and negative charges balance out to zero, resulting in an electrically neutral compound.

30
Q

1.7 Balencing Chemical Equations

What is a chemical equation?

A

A chemical equation is a way to represent a chemical reaction

31
Q

1.7 Balencing Chemical Equations

What is the chemical equation rule?

A

Atoms are not created of destroyed during a chemical reation

That is why you can only change the subscript not number

32
Q

1.7 Balencing Chemical Equations

Balence this Equation:
C₃H₈ + O₂ = CO₂ + H₂O

A

C₃H₈ + 5O₂ = 3CO₂ + 4H₂O

(Combustion of Propane)

33
Q

1.7 Balencing Chemical Equations

Balence this Equation:
H₂ + O₂ = H₂O

A

2H₂ + O₂ = 2H₂O

(Formation of Water)

34
Q

1.7 Balencing Chemical Equations

Balence this Equation:
Fe + O₂ = Fe₂O₃

A

4Fe + 3O₂ = 2Fe₂O₃

(Rust Formation)

35
Q

1.7 Balencing Chemical Equations

Balence this Equation:
KClO₃ = KCl + O₂

A

2KClO₃ = 2KCl + 3O₂

(Decomposition of Potassium Chlorate)

36
Q

1.7 Balencing Chemical Equations

Simplify this equation:
Ag⁺¹ (No₃)⁻¹

A

= Ag (No₃)

⁺¹ and ⁻¹ cancel

Avoid writing 1’s

37
Q

1.8 Conservation of Mass

What is a physical change?

A

A physical change is a reaction where reactants and products remain the same elements after a reaction but their state of matter changes

E.g. Ice melts to water
Still H2O just in a different sate of matter

38
Q

1.8 Conservation of Mass

What is the law of Conservation?

A

In any chemical reaction, the total mass of the reactants is equal to the total mass of the products.

(Reactants mass = Products mass)

(burn wood, the weight of the ash and gases produced equals the weight of the original wood and oxygen)

39
Q

1.8 Conservation of Mass

What is a chemical change?

A

A chemical change is a reaction where atoms re-arragnge themselves to form new chemical resuits (new elements)

E.g. Maginium and Oxygen form mahgnesium oxide which is a new element

40
Q

1.9 Types of Chemical Reactions

What is a synthesis/combination reaction?

A

A synthesis/combination reaction involves the combination of two or more reactants to form a single product

41
Q

1.9 Types of Chemical Reactions

What is a decomposiotion reaction?

A

A decomposition reaction involves the breakdown of a single compound into two or more simple substanses

42
Q

1.9 Types of Chemical Reactions

What is a compustion reaction?

A

A compustion reaction involves the reapid reaction of a substance with oxygen.

Typically produces heat or light

43
Q

1.9 Types of Chemical Reactions

What is an Oxidation reaction?

A

An oxidation reaction refers to the process by which metals react with oxidising agents (oxygen)

Typically occurs on the surface of metals

44
Q

1.10 Rates of reactions

What is the rate of a reaction?

A

The rate of a reaction refer to how quickly a reactant is used up or a new product is formed in a chemical reaction.

45
Q

1.10 Rates of reactions

How do you know when a chemical reaction has occured?

A

For a chemical reaction to happen:
* reactant particles must collide with eachother
* the particle must have enough energy for them to react

46
Q

1.11 Factors affecting reaction rates

What are the conditions of a faster reaction rate?

(5)

A
  • Decrease volume
  • increasing amount of reactant
  • increaing temperature
  • Increasing surface area
  • Stirring
47
Q

1.12 metals and metalic bonding

What is metalic bonding?

A

When a metal atom loses an electron/s forming a cation (pos ion)

48
Q

1.12 metals and metalic bonding

How are metal ions arranged?

A

Metal Ions are arranged in a closely packed lattice, they are in fixed positions

**Lattice = the fixed position of metals **

49
Q

1.12 metals and metalic bonding

What is the detocalised sea of electrons?

A

The detocalised sea of electrons is the outer layer electrons on the metal atoms that seperate the atom

50
Q

1.12 metals and metalic bonding

How does a high melting point relate to metalic bonding?

A

A high melting point in metals indicates strong metallic bonding due to positive metal ions being surrounded by a “sea of delocalized electrons”which hold a strong attraction that requires a lot of energy to break, leading to a high melting point.

Bonding comes from forces holding ions together in lattice structure

51
Q

1.12 metals and metalic bonding

How does lustrous/shiny appearence relate to metalic bonding?

A

The lustrous or shiny appearance of metals is due to the “sea of delocalized electrons” ability to absorb and re-emit light efficiently.

The lustrous or shiny appearance of metals** does not hinder metallic bonding**; instead, it is a result of metallic bonding itself.

52
Q

1.12 metals and metalic bonding

How does a metal being malleable relate to metalic bonding?

A

The malleability of metals, is a result of metallic bonding.
In metallic bonding, the positive metal ions are surrounded by a “sea of delocalized electrons”, which allows the ions to slide past each other without breaking the overall bond. This flexibility in the lattice structureenables metals to deform without shattering.

Malleable - ability to be hammered or rolled into thin sheets

53
Q

1.12 metals and metalic bonding

How does a metal being a good conductor of electricity impact metalic bonding?

A

The good electrical conductivity of metals is due to metallic bonding.
In metallic bonding, delocalized electrons can move freely throughout the metal lattice. These free-moving electrons allow metals to easily conduct electric current when a voltage is applied.

54
Q

1.12 metals and metalic bonding

How does a metal being a good conductor of heat impact metalic bonding?

A

The good thermal conductivity of metals is due to metallic bonding.
In metallic bonding, delocalized electrons can move freely throughout the metal lattice. These free-moving electrons transfer kinetic energy efficiently, allowing heat to spread quickly through the metal.

55
Q

1.7 Balencing Chemical Equations

Balence this Equation:
CO₂ + H₂O = C₆H₁₂O₆ + O₂

A

6CO₂ + 6H₂O = C₆H₁₂O₆ + 4O₂

(Photosynthesis Reaction)

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