Atomic Structure - Topic 1 Flashcards
(c) What is meant by the term Atom? (1.14)
. An atom is the basic building block of all matter in chemistry and can be found alone, or as a combination
. The smallest particle of an element
. An atom consists of:
- Protons
- Neutrons
- Electrons
. P + N together are the nucleus with E’s orbiting around it
(c) What is meant by the term Molecule? (1.14)
. A molecule is a group of two or more atoms chemically combined to make a identifiable unit which retains the properties and composition of the substances
(c) Protons (1.15)
. Protons
- Mass = 1
- Charge = +1
- Location = In the nucleus
. The number of protons in the nucleus determines the name of the atom
. If there is more protons than electrons the particle in an ion. (Ca+ ion = Positive ion)
(c) Neutrons (1.15)
. Neutrons
- Mass = 1
- Charge = 0
- Location = In the nucleus
(c) Electrons (1.15)
. Electrons
- Mass = 1 / 1840
- Charge = -1
- Location = In the shells
Fun facts about Atoms :D
. More electrons = Negative charge
. More protons = Positive charge
. To find N.O of electrons it is just the same as the N.O of protons unless it is an isotope
. N.O of neutrons is Mass N.O - Atomic N.O
(c) How can an atom be neutral (1.15)
. An atom can become neutral if the number of protons is equal to the number of electrons
(c) What is meant by the term Atomic number? (1.16)
. The number of protons in an element
. (The bottom or top number depending on the periodic table)
(c) What is meant by the term Mass number? (1.16)
. The number of protons and neutrons in an element
. (The bottom or top number depending on the periodic table)
(c) What is meant by the term Isotope? (1.16)
. Isotopes are atoms of the same element with the same number of protons but a different number of neutrons
¹²C, ¹³C, ¹⁴C…
(c) What is meant by the term relative atomic mass (Ar)? (1.16)
. The relative atomic mass is the average mass of all different isotopes of an element (accounting for the abundance of isotopes)
. It is on a scale where it is equal to 1/12th the mass of an atom carbon-12
(c) Be able to calculate the relative atomic mass (Ar) of elements from isotopic abundances (1.17)
. Relative atomic mass (Ar) = Total mass of all atoms / Total number of all atoms
(d) Understanding how elements are arranged in the periodic table (1.18)
. Elements are ordered by the size of their Atomic Numbers horizontally
. They are ordered vertically, in groups (columns) going from left to right, going from 1 to 7 (Then 0)
. They are ordered horizontally, in periods (rows) going downwards from 1 at the top to 7 at the bottom
(d) How to find the abundance of electrons in an atom (1.19)
. To find the abundance electron you can just use the atomic number
(d) Understanding how to deduce the electron configurations of the first 20 elements based on their position on the table (1.19)
. Atoms have 3 shells
- The 1st can store 2 electrons
- The 2nd can store 8 electrons
- The 3rd shell and so on can also hold
only 8 electrons
. To find the electron configuration, use the atomic number and distribute electrons into shells based on their capacity.
- This can either be represented by electron notation _ , _ , _ or by diagrams
(d) Atomic number and Electron configuration of Hydrogen (1.19)
. Hydrogen
- Atomic Number = 1
- Electron config = 1
(d) Atomic number and Electron configuration of Helium (1.19)
. Helium
- Atomic number = 2
- Electron config = 2
(d) Atomic number and Electron configuration of Lithium (1.19)
. Lithium
- Atomic number = 3
- Electron config = 2,1
(d) Atomic number and Electron configuration of Beryllium (1.19)
. Beryllium
- Atomic number = 4
- Electron config = 2,2
(d) Atomic number and Electron configuration of Boron (1.19)
. Boron
- Atomic number = 5
- Electron config = 2,3
(d) Atomic number and Electron configuration of Carbon (1.19)
. Carbon
- Atomic number = 6
- Electron config = 2,4
(d) Atomic number and Electron configuration of Nitrogen (1.19)
. Nitrogen
- Atomic number = 7
- Electron config = 2,5
(d) Atomic number and Electron configuration of Oxygen (1.19)
. Oxygen
- Atomic number = 8
- Electron config = 2,6
(d) Atomic number and Electron configuration of Fluorine (1.19)
. Fluorine
- Atomic number = 9
- Electron config = 2,7
(d) Atomic number and Electron configuration of Neon (1.19)
. Neon
- Atomic number = 10
- Electron config = 2,8
(d) Atomic number and Electron configuration of Sodium (1.19)
. Sodium
- Atomic number = 11
- Electron config = 2,8,1
(d) Atomic number and Electron configuration of Magnesium (1.19)
. Magnesium
- Atomic number = 12
- Electron config = 2,8,2
(d) Atomic number and Electron configuration of Aluminium (1.19)
. Aluminium
- Atomic number = 13
- Electron config = 2,8,3
(d) Atomic number and Electron configuration of Silicon (1.19)
. Silicon
- Atomic number = 14
- Electron config = 2,8,4
(d) Atomic number and Electron configuration of Phosphorus (1.19)
. Phosphorus
- Atomic number = 15
- Electron config = 2,8,5
(d) Atomic number and Electron configuration of Sulfur (1.19)
. Sulfur
- Atomic number = 16
- Electron config = 2,8,6
(d) Atomic number and Electron configuration of Chlorine (1.19)
. Chlorine
- Atomic number = 17
- Electron config = 2,8,7
(d) Atomic number and Electron configuration of Argon (1.19)
. Argon
- Atomic number = 18
- Electron config = 2,8,8
(d) Atomic number and Electron configuration of Potassium (1.19)
. Potassium
- Atomic number = 19
- Electron config = 2,8,8,1
(d) Atomic number and Electron configuration of Calcium (1.19)
. Calcium
- Atomic number = 20
- Electron config = 2,8,8,2
(d) Identifying if an element is a Metal or a Non-Metal using the periodic table (1.21)
. To do this draw a staircase, with the top step being at the bottom of boron and the last step being under Astatine and Radon
(d) Understanding how the electron configuration of main group elements are related to there position on the periodic table (1.22)
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. Elements that are inside the same group on the Periodic Table will share similar chemical properties
. This is because they have the same number of electrons so they will bond and react similarly
. The group number of an element which is given on the Periodic Table shows the number of electrons in the outer shell
- although is in Group 0, it has only one
shell, that can only hold 2 electrons
(d) Periodic table reactivity (My own addition)
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. Use the group number to predict how elements will react as the number of outer shell electrons in an element influences how the element reacts.
Therefore, elements in the same group react similarly
(d) Periodic table reactivity (My own addition)
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By observing the reaction of one element from a group, you can predict how the other elements in that group will react
By reacting two or more elements from the same group, you can establish trends in reactivity in that group by observing the reactions
(d) Periodic table reactivity (My own addition)
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For instance, lithium, sodium and potassium are in Group 1 and can all react with elements in Group 7 to form an ionic compound
Also, the Group 1 metals become more reactive as you move down the group meanwhile, the Group 7 elements show a decrease in reactivity moving down the group
(d) How to identify the charges of elements using the periodic table (My own addition)
. To identify the charges of elements write above the group numbers, going from left to right;
G1 = +1
G2 = +2
G3 = +3
G4 = +4
G5 = -3
G6 = -2
G7 = -1
G8 = 0
