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

1
Q

Write a Definition of a Atom?

A
  • A Atom is a the smallest part of an element that can exists.
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2
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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3
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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4
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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5
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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6
Q

How many electrons does The 1st, 2nd , 3rd Shells Each hold?

A
  • The 1st Shell Holds 2 Electrons
  • The 2nd and 3rd Shell Both Hold 8 electrons.
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7
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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8
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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9
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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10
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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11
Q

What Equations Tells you the number of neutrons?

A
  • Mass Number - Atomic Number
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12
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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13
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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14
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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15
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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16
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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17
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.

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18
Q

Write a Definition of a Compound?

A
  • A Compound is a Substance with 2 or more different elements held for 2 Chemical bonds.
19
Q

How Do you Separate a Compound?

A
  • The Only way to separate a Compound into elements is by using a Chemical Reaction.
20
Q

In 3 Steps How do You Balance a Chemical Equation?

A
  • 1) Write down the number of atoms for each element on both sides of the equation.
  • 2) Add big numbers in front of the compounds to make the atoms equal but start with metals, Non-metals and leave oxygen and hydrogen at last.
  • 3) Recount atoms to ensure balance and double check again.
21
Q

Name 2 Rules Of Chemical Equations?

A
  • 1) Can’t Change the Little Numbers.
  • 2) Keep whole Numbers.
22
Q

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

A
  • A Mixture consist of 2 or more elements or compounds not chemically combined together.
  • For example air.
23
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.
24
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.
25
Q

Write Down the mnemonic to Remember the History of the Atom?

A
  • Jolly - ( John Dalton) - Solid Spheres
  • Jimmy (J.J Thompson) - Plum Pudding Model
  • Eats - (Ernest Rutherford) - Nuclear model
  • Noodles ( Neil’s Bohr) - Adapting Nuclear model
  • Joyfully (James Chadwick)
26
Q

What Does the Plum Pudding Model Suggest?

A
  • The plum pudding model suggested the atom is a ball of positive charge with negative electrons embedding it.
27
Q

What Did Ernest Rutherford Do and what did it lead to?

A
  • Ernest Rutherford took positive charged particles and fired it at a thin sheet of gold.
  • Alpha Particle scattering led to the conclusion that the mass of an atom was concentrated at the centre and the nucleus was charged.
28
Q

What was Neil’s Bohr model and what did it suggest?

A
  • Neil’s Bohr model was the nuclear model
  • It suggested that electrons orbit the nucleus at specific distances.
29
Q

What Did James Chadwick Provide?

A
  • James Chadwick provided evidence to show the existence of neutrons without the nucleus.
30
Q

Who created the Period Table and What Was Special About it?

A
  • Mendeleev Created the period table.
  • It was Special as New Elements Were discovered and Mendeleev discovered it and filled in the gaps.
31
Q

What Does the Group Number tell you and What Happens When you go down the Group?

A
  • The group Number tells you how many protons fit in the outmost shell.
  • When you go down the groups the Elements become more reactive with water.
32
Q

Where are Metals, Transition Metals and Non-Metals Found?

A
  • Metals and Transition metals are found on the left hand side of the periodic table.
  • Non - Metals Are found in the right hand side of the periodic table.
33
Q

Name 2 Differences Between Metals and Non - Metals?

A
  • Metals are Malleable and Good Conductors of Heat and Electricity.
    -Non - Metals are Brittle and Bad conductors of heat and electricity.
34
Q

What are Transition Metals?

A
  • Transition metals are typical metals that have some extra properties for example they can form more than one ion.
35
Q

What are Group 1 Metals Know as and What happens in terms of Reactivity?

A
  • The group 1 Metals are know as alkali metals.
  • The Reactivity increases as you go down the group.
36
Q

Why does the reactivity increase as you go down group 1?

A
  • It increases as They all have 1 electron in the outmost shell but as you go down the electron is further form the nucleus ands It more easier for it to lose that electron.
37
Q

What Happens If a alkali metal Reacts with water?

A
  • When the alkali metal is put in water it reacts vigorously to produce metal hydroxide and hydrogen gas.
38
Q

What Happens If a alkali metal reacts with chlorine?

A
  • They react vigorously when heated in chlorine gas and form white metal chloride salts.
39
Q

What Happens If a alkali metal reacts with Oxygen?

A
  • When alkali metals react with oxygen they form metal oxides.
  • However the type of oxide depends on the metal.
40
Q

What Is group 7 called and what do they have in common?

A
  • Group 7 is called Halogens
  • They have similar reactions because they all have 7 electrons in their outer shell.
  • They are also non-metal and consist of molecules made of pairs of atoms.
41
Q

How do Chlorine, bromine and iodine react with metals and non-metals?

A
  • Chlorine, bromine and iodine react with metals they form ionic bonds and transfer electrons.
  • Chlorine, bromine and iodine React with Non- Metal They form Covalent bonds and share electrons.
42
Q

What are the trends in Group 7 and How does Displacement reaction work?

A
  • The melting and Boling Point increases and the reactivity decreases.
  • A More reactive halogen can displace a less reactive halogen from an aqueous solution of its salt.
43
Q

What’s Group 0 Called and What similarities do they all have?

A
  • Group 0 Is called the noble gases.
  • They are colourless, Have full outer shells so they aren’t reactive, They are Non-flammable.
44
Q

What is the trend of Group 0?

A
  • The boiling point increases as you go down