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Chemistry- Combined Science > C:1 Atomic Structure and The Periodic Table Paper 1 > Flashcards

C:1 Atomic Structure and The Periodic Table Paper 1 Flashcards

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1
Q

Write a Definition of a Atom?

A
  • A Atom is a Neutral Particle made up of Protons and Neutron in the nucleus with electrons surrounding the nucleus.
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2
Q

How small are atoms and what substances contains Atom?

A
  • All Substances Contain Atoms.
  • They are really small to small to see.
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3
Q

What’s the Atomic Radius of a Atom?

A
  • The Atomic Radius of a Atom is About 0.1 Nanometres.

 

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4
Q

What’s Charge would the Nucleus be and what fills half of the mass of the Atom?

A
  • It Would be Positive charge because of The Protons.
  • Almost the whole mass of the atom is in the nucleus.
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5
Q

Write a Definition of The Nucleus (Atom)?

A
  • The Nucleus is the center of the atom containing protons and neutrons.
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6
Q

Write a Definition of an Electron?

A
  • a Electron is a Negatively charged particle that orbits the nucleus of a Atom.
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7
Q

Write a Definition of Energy Levels/Electron Shell?

A
  • Energy Levels/Electron Shell is a Region of an Atom That Contains Atoms.
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8
Q

What do Electrons and Describe Their Mass?

A
  • Electrons move around the nucleus in electrons shells.
  • Electrons Have Almost No Mass
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9
Q

What’s the Relative Mass and Relative charge of a Proton?

A
  • The Relative Mass of a Proton is 1.
  • And The Relative Charge is +1.
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10
Q

What’s the Relative Mass and Relative charge of a Neutron?

A
  • The Relative Mass of a Neuron is 1.
  • And The Relative Charge is 0.
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11
Q

What’s the Relative Mass and Relative charge of a Electron?

A
  • The Relative Mass of a Electron is Very small.
  • And the Relative Charge is -1.
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12
Q

What Does the Atomic Number of a Element tell you?

A

It Tells us The Number of Protons and Electrons.

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13
Q

What Equations Tells you the number of neutrons?

A
  • Mass Number - Atomic Number
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14
Q

Atoms have No (____________________) they are (______________).

A
  • Overall charge and Neutral.
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15
Q

Write a Definition of an Ion?

A
  • A Ion is a Charged Particle formed when one or more electrons are lost or gained from an atom or molecule.
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16
Q

The (__________) of Electrons is the same (_______) as the charge on the (___________) but opposite so they cancel out.

A
  • Charge,Size and Proton
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17
Q

What Happens if a Atom has the Same amount of Protons and Electrons?

A
  • The Atom won’t have a Positive or Negative Charge it will be Neutral.
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18
Q

What Would Happen If A Ion gains a Extra Electron and What Would Be The Charge of The Ion?

A
  • If a Ion Gains a Extra Electron It Would be a Negative Ion.
  • and The Overall Charge will 1 -
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19
Q

What Would Happen if a Ion loses and What would be the Charge of the Ion?

A
  • If a Ion Loses a Electron then it would be a Positive Ion.
  • And the Overall Charge will be 1+.
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20
Q

Write a Definition of a Anion?

A
  • A Anion is a Particle with a Negative Charge Formed when one or more electron are Gaineded.
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21
Q

Write a Definition of a Cation?

A
  • A Cation is a Particle with a Positive Charge Formed When one Or More Electron are Lost.
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22
Q

Write a Definition of an Electron?

A
  • a Electron is a Negatively charged particle that orbits the nucleus of a Atom.
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23
Q

What’s The Smallest Part of a Element and What Thing Decides What Element it is?

A
  • The Smallest Part of a Element is that you can have a single Atom of the element.
  • The Number of Protons Decides what type of of atom it is.
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24
Q

What are All Atoms similarities and differences and how can elements be represented?

A
  • All Atoms have the same number of protons.
  • But they are Different Elements with Different number of Protons.
  • Elements can Be Resperenteded by 1 0r 2 Letter symbol.
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25
Q

Write a Definition of Isotope?

A
  • A Isotope is a Different Form of the Same Element which has atoms With The Same Number of Protons but a different number of neutrons and it has a different mass number.
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26
Q

What Would Happen if a Element has A Number of Isotopes?

A
  • If a Element has a Number of Isotopes then it can be describe using Relative Atomic Mass (Ar) Instead of a Mass Number.
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27
Q

Write a Definition of Relative Atomic Mass (Ar) and What is The (Ar) of a Element the Same As?

A
  • The (Ar) is The Average mass of the atoms of An element Measured to Relative Mass of One Atom Of Carbon -12.
  • The (Ar) of an element is the same as its mass number in the period table.
28
Q

Write a Definition of Relative Formula Mass (Mr) and How Is It Calculated?

A
  • Mr is all the relative atomic masses of the Atom in a Compound Added Together.
  • Ar is Worked Out from the Different Masses and Abundances of Each Isotope.
29
Q

What’s The Formula to Work out The Relative Atomic Mass of an Element?

A

Sum of ( Isotope Abundance x Isotope mass Number) ÷ Sum of Abunces of all isotopes.

30
Q

Write a Definition of a Compound?

A
  • A Compound is a Substance made up of Atoms of at Least 2 Different Elements,Chemically Joined Together.
31
Q

Write a Definition of a Organic Compound?

A
  • A Organic Compound is a Chemical Compound That contains carbon atoms.
32
Q

What Happens To The Atoms in a Chemical Reaction to Form Compounds and How Do you Separate a Compound?

A
  • The atoms of each element are in fixed Proportions in the Compound.
  • The Atom are Held together by chemical bonds.
  • The Only way to separate a Compound into elements is by using a Chemical Reaction.
33
Q

How Can Compound Be Represented and What are they made up of?

A
  • Compounds can Be Repressed By Formulas.
  • The Formula are made up of Element Symbols in the Same Properties as the Elements in The Compound.
34
Q

What Do Number In The Element Symbol Tells Us and Give a Example?

A
  • The Numbers In Different Element Symbols Tells Us how Many elements are in the compound.
  • For Example: Carbon Dioxide CO2 Is a Compound made from a Reaction Between carbon and oxygen.
  • It Contains 1 carbon atom and 2 oxygen atoms.
35
Q

What Might Formulas Also Have and What Does the Number Outside The Bracket Show and Give a Example?

A
  • Formulas Might Also Have Brackets.
  • For Example: Ca(OH)2.
  • The little number 2 outside the Bracket means there’s is 2 of everything inside the bracket.
  • So There is 1 Calcium atom and 2 Oxygen and 2 Hydrogen atoms.
36
Q

What’s The Chemical symbol for Ammonia,Sodium chloride,carbon monoxide and Hydrochloric Acid?

A
  • Ammonia - NH3
  • Sodium Chloride - NaCl
  • Carbon Monoxide - CO
  • Hydrochloric Acid - HCI
37
Q

What’s the Chemical symbol, For Calcium Chloride,Sodium Carbonate and Sulfuric Acid?

A
  • Calcium Chloride - Ca Cl2
  • Sodium Carbonate - Na 2 CO3
  • Sulfuric Acid - H2SO4
38
Q

How do you present a Chemical Reaction?

A
  • The Only Way to Present a Chemical Reaction is by using a Word Equation.
39
Q

Write a Definition of Reactants
And What’s On The Left Hand Side (LHS) Of a Chemical Word Equation?

A
  • Reactants Are Substances that reacts in a Chemical Reaction.
  • On The Left Hand Side (LHS) of a Chemical Equation is Reactants.
40
Q

Write a Definition of Products and What’s On The Right Hand Side (RHS) of a Chemical Word Equation?

A
  • Products are Substances that form in a Chemical Reaction.
  • On the Right Hand Side (RHS) of a Chemical equation is Products.
41
Q

What Must always Be the same in front of the atom on boths Sides?

A
  • It Must have the Same Number in front of it.
42
Q

In 3 Steps How do You Balance a Chemical Equation?

A
  • 1) First we Need to Count the Number Of atoms Of Each Element On The (LHS) And (RHS) Of the equation.
  • 2) Next Find an element that doesn’t balance and put a Number in Front of it.
  • 3) If the Equation isn’t Balanced Swap it with another Number and keep doing that until the equation is balanced.
43
Q

Name 2 Rules Of Chemical Equations?

A
  • 1) Can’t Change the Little Numbers.
  • 2) Keep whole Numbers.
44
Q

Write a Definition of a Mixture and Give a Example of a Mixture?

A
  • A Mixture is a Substance made from 2 or more elements or compounds that aren’t chemically bonded to each other.
  • For Example : Air is a Mixture of gases Mainly Nitrogen,oxygen,carbon dioxide and argon.
45
Q

Name 5 Methods that Separate Mixtures?

A
  • 1) Filtration.
  • 2) Crystalistion.
  • 3) Fractional Distillation.
  • 4) Simple Distillation.
  • 5) chromatography.
46
Q

Write a Definition of Physical Methods?

A
  • Physical Methods Are Methods that involve chemical Reactions but don’t form any new substances.
47
Q

What are Properties and What are the Properties of a Mixture?

A
  • Properties describe what a substance is Like and How it Behaves.
  • The Properties of a Mixture are just a Mixture
48
Q

Write a Definition of Chromatography?

A
  • Chromatography is an Analytical Method used to separate the substances in a Mixture based On How the components interact with a mobile phase and stationary Phase.
49
Q

In 7 Steps how do you do Paper Chromatography (PRACTICAL)

A
  • 1)Use a Pencil to Draw a line near the bottom of a Sheet of filter paper and Add a spot of ink to the line.
  • 2) Pour a Small amount of solvent into a beaker so it form a shallow layer.
  • 3) The Solvent Used depends on what’s being Tested Some compounds dissolve well in water but sometimes other solvents like ethanol are needed.
  • 4) Place the Sheet in the Beaker of Of Solvent But make sure the Ink isn’t Touching the Solvent.
  • 5) Place a Lid on top of the container to stop the solvent Evaporating.
  • 6) The Solvent seeps up the pepr carrying the ink with it.
  • 7) When the solvent has nearly reached the top of the paper take the paper out of the beaker and leave it to dry.
50
Q

Write a Definition of Chromatogram and Solute

A
  • A Chromatogram is The Pattern of Spots formed as a result of separating a mixture using chromatography.
  • A Solute is a substance dissolved in a solvent to make a solution.
51
Q

rite a Definition of Rf Value ?

A
  • Rf Value is the ratio between the distance travelled by a dissolved substance and the distance traveled by a solvent.
52
Q

In Chromatography What’s the Mobile phase and Stationary phase?

A
  • The Mobile phase is a gas or liquid where molecules are able to move.
  • the Stationary Phase is a Solid or really thick liquid where molecules are unable to move.
53
Q

Write a Definition of Solvent and Solvent Front?

A
  • A Solvent is a liquid in which another substance can be dissolved.
  • A Solvent Front is The point the solvent has reached up the filter paper during Chromatography.
54
Q

What Happens During Chromatography And what will Each dye Do?

A
  • During Chromatography Each different dye dye in the ink moves up the paper at different speeds and this separates the dyes.
  • Each dye will form a spot in a Different Place so there should be 1 spot for each dye in the ink.
55
Q

What Happen to the Dyes that don’t dissolve in the Solvent?

A
  • They Will stay on the pencil line.
56
Q

Write a Definition of a Solution and Mixture?

A
  • A Solution is a Liquid That has a soluble Solid that does dissolves.
  • A Mixture is a Liquid that has a solid that doesn’t dissolve.
57
Q

(_______________) andn (_______________________) Can be used to separate insoluble solids Like (____________).

A
  • Filtration ,Crystallisation and rock salt.
58
Q

Write a Definition of Insoluble and Soluble?

A
  • Insoluble is a Substance that does not dissolve in a particular solvent.
  • Soluble is a Substance that does Dissolves in a Solvent.
59
Q

In 4 Steps How do You Use Filtration to Separate insoluble Solids from Liquids (PRACTICAL)?

A
  • 1) Fold The Filter paper into a Cone Shape and Put the Filter paper in a funnel.
  • 2) Pour the Mixture into the filter paper.
  • 3) Make sure the mixture doesnt go above the filter paper.
  • 4) The liquid passes through the paper into the beaker the Solid is left behind in the filter paper.
60
Q

Name 2 Methods to Separate Soluble Solids from Solutions?

A
  • 1) Evaporation.
  • 2) Crystallisation.
61
Q

In 3 Steps How do you use Evaporation to separate soluble Solids (PRACTICAL)?

A
  • 1) Slowly Heat The Solution in an Evaporating Dish the Solvent Will Evaporate.
  • 2) Eventually the Crystals wii start to form.
  • 3) Keep Heating until all you have left are dry crystals.
62
Q

In 4 Steps How do you Use Crystallisation to Separate Soluble Solids (PRACTICAL)?

A
  • 1) Gently Heat the solution in an Evaporating Dish some of the Solvent will Evaporate.
  • 2) Once Some of The Solvent has Evaporated or when you see crystals start to form stop heating it and leave the solution to cool.
  • 3) The Salt should start to form crystals.
  • 4) Filter the Crystals out of the solution And leave them in a warm place to dry.
63
Q

What is Rock Salt and In 4 Steps How do You Separate Them?

A
  • Rock Salt is a Mixture of Salt and sand salt dissolves in water but sand doesn’t.
  • 1) Grind the Mixture to make sure the salt crystals are small so they will dissolve easily.
  • 2) Put the mixture in water and stir the salt will dissolve but the sand wont.
  • 3) Filter the mixture but the Grains of sand won’t fit through the tiny holes in the filter paper so they will have to collect on the paper instead.
  • 4) Use evaporation or Crystallisation so you end up with dry crystals.
64
Q

Name 2 Methods to separate mixtures which contain Liquids and Write a Definition of Simple Distillation?

A
  • 1) Simple Distillation.
  • 2) Fractional Distillation.
  • Simple Distillation is a Way of separating a liquid out from a mixture if there are large differences in the boiling points of a substance..
65
Q

In 8 Steps how do You Use Simple Distillation to separate Solutions (PRACTICAL)?

A
  • 1) First evaporate the liquid by heating this turns the liquid into vapour.
  • 2)

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