Atom Flashcards
Define the term ‘atom’
An atom is the smallest part of an element that can still be recognised as that element
How do you know if a chemical equations is balanced
The number of atoms of each element on the reactants side will be equal to the number of atoms of each element on the products side
Define the term ‘electron’
An electron is a tiny particle with a negative charge. Electrons orbit the nucleus of atoms or ions in shells
Define the term ‘proton’
A proton is a tiny positive particle found inside the nucleus of an atom
Define the term ‘neutron’
A neutron is a dense particle found in the nucleus of an atom. It is electrically neutral, carrying no charge.
Define the term ‘shell’
A shell is an area in an atom, around its nucleus, where electrons are found.
Finish the sentence
All substances are made of tiny particles called ____________
All substances are made of tiny particles called atoms
Name the sub-atomic particles found in the atom
Protons, Neutrons and Electrons are sub-atomic particles are found in the atom
Name the sub atomic particles that make up the nucleus of an atom
Protons and Neutrons are found in the nucleus of an atoms
Where is the nucleus in an atom
The nucleus is in the middle of the atom
Where are the electrons found in
Electrons are found in electron shells, outside of the nucleus
What is an ion
An ion is a charged particle produced by the loss or gain of electrons
Define the term ‘element’
An element is a pure substance containing only one type of atom. An element cannot be broken down chemically into any simpler substance.
Define the term ‘compound’
A compound is a pure substance made when two or more different types of atoms are chemically bonded together.
Define the term ‘mixture’
A mixture is made up of two or more different substances that are not chemically bonded together
Why is a mixture easy to separate
A mixture is easy to separate as the substances that make up the mixture are not chemically bonded together.
Define the term ‘pure’
Pure - a material made up of one type of substance.
Define the term ‘molecule’
A particle made up of at least two atoms chemically bonded together by covalent bonds
State the relative mass of a proton
The relative mass of a proton is 1
State the relative mass of a neutron
The relative mass of a neutron is 1
State the relative mass of an electron
State the relative mass of a electron is 1/2000
Finish the sentence: Most of an atom is _________
Most of an atom is empty space
State the relative charge of the sub-atomic particles
Proton = +1
Neutron = 0
Electron = -1
Why does the nucleus have a positive charge
The nucleus is positively charged as the only charge in the nucleus are the protons which are positively charged. The neutrons have no charge.
Draw the electronic structure (dot and cross diagram) of sodium
State it’s electron configuration
Sodium - 2, 8, 1
Identify the mass number and the atomic number
https://d17hukvrbysd4e.cloudfront.net/blogImages/atomic-number-and-mass-number.jpg
Define the term ‘mass number’
The mass number is the total number of protons and neutrons in the nucleus of a given atom.
Define the term ‘atomic number’
The atomic number is the total number of protons in the nucleus of a given atom
How would you find out how many neutrons an atom has.
Number of neutrons = mass number - atomic number
What does the atomic number determine
The atomic number determines the type of atom. (For example, any atoms with 6 protons are carbon atoms)
Explain why an atom is uncharged
An atom is uncharged as it has an equal number of positively charged protons and negatively charged electrons. These charges cancel out.
Define the term isotope
Isotope - Atoms that have the same number of protons but a different number of neutrons
Give an example of Isotopes
Carbon-12, Carbon-13, Carbon-14, Chlorine-35, Chlorine-37
How are isotopes named
Isotopes are named by their mass number. For example Carbon-12 has a mas number of 12 (6 protons and 6 neutrons)
Work out the number of protons, neutrons and electrons in:
Carbon-12
Carbon-13
Carbon-14
Carbon-12 : 6 protons, 6 electrons, 6 neutrons
Carbon-13 : 6 protons, 6 electrons, 7 neutrons
Carbon-14: 6 protons, 6 electrons, 8 neutrons
When do you use relative atomic mass instead of mass number
The relative atomic mass is used when referring to the element as a whole
Define the term ‘ relative atomic mass’ - A (subscript r)’
The relative atomic mass is the average mass of the atoms of an element, taking into account the different masses and abundances of all isotopes that make up the element.
State the formula for relative atomic mass
relative atomic mass (A subscript r) = sum of (isotope abundance x isotope mass number) / sum of abundances of all the isotopes
Copper has two stable isotopes. Cu-63 has an abundance of 69.2% and Cu-65 has an abundance of 30.8%. Calculate the relative atomic mass of copper to 1 d.p.
relative atomic mass (A subscript r) = sum of (isotope abundance x isotope mass number) / sum of abundances of all the isotopes
relative atomic mass = (69.2 x 63) + (30.8 x 65)/69.2+30.8
= 4359.6 + 2002/100
= 6361.6/100
= 63.616 = 63.6 (to 1.d.p)
What term do you use (instead of mass number) when referring to the element as a whole
The relative atomic mass is used when referring to the element as a whole
Complete the sentence
Isotopes exist in different _________ (some isotopes are more common than others)
Isotopes exist in different quantities (some isotopes are more common than others)
What can energy levels also be called
Energy levels can be called ‘shells’
How many electrons can each shell hold
1st shell - 2
2nd shell - 8
3rd shell - 8 etc.
What does the period number tell you?
In the periodic table, the period number is equivalent to the number of electron shells an atom contains
What does the group number tell you
In the periodic table, the group number shows the number electrons an atom has in it’s outer most shell.
Which shell is the highest energy level
(1st, 2nd, 3rd shell)
The third shell is the highest energy level.
Finish this sentence
As the distance from the nucleus increases, the _____ in the ______/_________ also increases
As the distance from the nucleus increases, the energy in the energy shell/electron also increases.
What type of ions do metals form
Metals form positive ions
What type of ions do non-metals form
Non-metals form negative ions
What do metals need to do in order to form positive ions
A metal loses electrons to form positive ions
What do NON METALS need to do in order to form NEGATIVE ions
A non-metal needs to lose electrons to form positive ions.
Why do atoms react with other atoms
Atoms react with atoms, to gain, lose or share electrons from in order to achieve a full outer shell (noble gas configuration)
Draw the electronic structure of a sodium ion
(state it’s electronic configuration)
https://www.gcsescience.com/sodium-ion.gif
[2,8]+
Draw the electronic structure of an oxide ion
https://bam.files.bbci.co.uk/bam/live/content/z3tn4qt/small
[2,8]-
What do group 4 elements do in terms of electrons
Group 4 atoms share electrons
Group 4 atoms don’t form ions but share electrons and form compounds.
Why don’t noble gases need to form ions.
Noble gases do not need to form ions as they have a full outer shell (they all have 8 electrons in their outer shell, apart from helium which has 2). This means that they do not need to gain or lose (or share) electrons to achieve a full outer shell, to become stable.
Why are Noble Gases so unreactive
Noble gases are unreactive because they have a full outer shell (they all have 8 electrons in their outer shell, apart from helium which has 2). This means that they do not need reactions to lose or gain or share electrons to achieve a full outer shell
Where in the atom is majority of the mass.
Majority of the mass of an atom is in the nucleus
When fluorine becomes an ion, what is it called
When fluorine becomes an ion, it is called a fluoride ion
