Periodic table of elements Flashcards
What are the periods of the periodic table
The rows
What are the groups of the periodic table
The columns
What is group 1 of the periodic Table known as
Alkali metals
What is group 2 of the periodic table known as
Alkaline earth metals
What is group 17 of the periodic table known as
Halogens
What is group 18 of the periodic table known as
Noble gases
What are groups 3 to 12 of the periodic table known as
Transitional metals
What are elements 58 to 71 in the periodic table known as
Lanthanoid
What are elements 90 to 103 in the periodic table known as
Actinides
What are lanthanides
Rare earth metals that are found in small quantities on earth
What are actinides
Most wot the known elements used in nuclear reactions and
What 4 areas is the periodic table divided into
s,p,d and f block
What are the s block elements
Group 1 and 2 elements
What are the p block elements
Group 13- group 18
What are the d block elements
Group 3- group 12
What are the f block elements
Lanthanides and actinides
What does the period indicate on the periodic table
The outermost energy level of the elements in that period
What happens to the atomic radius from left to right in a given period and why?
It decreases, because there is an increase in protons but the number of energy levels stays the same thus the electrons are drawn more by the nucleus with greater charge so the atom volume shrinks and atomic radii decreases
What happens to the atomic radius from top to bottom in a group and why ?
It increases, because as you go down a group the number of energy levels increases thus the number of inner electrons Increases and they shield the outer electrons from the force of attraction of the core thus the atom volume increases so that the atomic radius increases
What happens to the melting and boiling point from left to right in a period and why ?
It increases with metals and decreases with nonmetals.
Group 1 metals have one valence electron while group 2 metals have two thus the forces of attraction are stronger in group 2 elements. Group 13 elements have a strong covalent network structure which is stronger than the metal bonding in the group 1 and 2 metals. Group 14 metals have a much stronger covalent structure and bond than group 13 metals. Thus the melting point and boiling point increase for metals across a period from left to right.
Non metals generally exist as simple molecules (diatomic molecules and P4, S8) and mono atomic molecules (Ne and Ar) that are held together by weak intermolecular forces of attraction thus the melting and boiling points are low and they decrease from left to right
What happens to the melting and boiling point from top to bottom for a group
It decreases with metals and increases with nonmetals
Because as metal atoms become larger (their atomic radius increases) the forces of attraction between them decrease (the nucleus is further away from the outer electrons and have a weaker force of attraction on them) and thus the melting and boiling points are lower because you need less heat to overcome the forces.
However for non metals it is the opposite because the weak forces of attraction between diatomic molecules increases as the mass of the atom increases
What happens to density from left to right across the period
It increases for metals and decreases for non metals
Because metals are tightly packed in a metal crystal and held together by strong forces of attraction between the metal atoms. The more valence electrons the stronger the forces of attraction and the tighter the particles thus the higher the density.
In simple molecules and monatomic molecules there are weak attraction forces between the molecules that causes their density to decrease
What are the factors that influence ionisation energy
- The charge of the nucleus
- the distance of the electrons from the nucleus (atomic radius)
- the number of inner level electrons between the outer level electrons and the nucleus (screening effect)
- repulsion forces of electrons in the same orbital
What happens to the first ionisation energy from left to right across the period
It increases, because as you move from left to right across a period the number of energy levels stay the same however the charge of the nucleus increases thus the nucleus holds on more tightly to the outer electrons. This means you’ll need more energy to remove the electron thus the ionisation energy increases as you move from left to right across a period
What happens to density as you move from top to bottom in a group
The density increases because the atomic mass of the atoms increase
What happens to the first ionisation energy as you move from top to bottom in a group
It decreases, this is because as you go down a group a new energy level is added which means there is more inner electrons shielding the outer electrons from the force of attraction of the nucleus and the distance from the nucleus to the outer electrons is larger thus the force of attraction is weaker thus it’s easier to remove an electron.
What is the trend between metals and non metals relating to ionisation energies and thus what can we conclude
Metals have low ionisation energies (500-860 kJ.mol-1) whereas nonmetals have high ionisation energies (800-2380 kJ.mol-1). Thus we can conclude that it is expected for metals to form positive ions in chemical reactions
Why is the second ionisation energy higher than the first ionisation energy
This is because the positive ion attracts the electrons more strongly
What happens to electron affinity as we move from left to right in a period and why?
It becomes more negative, because from left to right nuclear charge increases which would mean that the new added electrons enter the outer Main energy level and they are drawn more strongly by the nucleus.
What is trend with metals and non metals relating to electron affinity
Metals have low (low negatives or positive) electron affinities and nonmetals have high (negative) electron affinities, this means that non metals are most likely to for negative ions during a chemical reaction
Which group had the highest electron affinity
Halogens because gaining an electron means they reach the octet structure which they are aiming for
What happens to electron affinity from top to bottom in a group
It decreases (less negative), because the newly added electrons are further away from the nucleus thus they experience a weaker force of attraction from the nucleus thus the electron affinity decrease
What happens to electronegativity for left to right in a period
Increases, because as we move along a period the atoms become smaller and the negative electrons are closer to the nucleus. the positive charge of the nucleus also bigger. This results in valence electrons being held tighter by the nucleus
What happens to electro negativity from top to bottom in a group
It decreases, because as more energy levels are added the inner electrons shield the outer electrons from the nucleus positive charge. This means hat the valence electrons are less tightly held and can easily be removed as we go down in a group.
In what ratio does oxygen bond with group 1 elements
2:1
In what ratio does oxygen bond with group 2 elements
1:1
In what ratio does oxygen bond with group 13 elements
2:3
In what ratio does oxygen bond with group 14 elements
1:2
In what ratio does oxygen bond with group 15 elements
2:5
In what ratio does oxygen bond with group 17 elements
2:1
What are the characteristics of a metal oxide
They are typical ionic crystalline solids, have high melting and boiling points, and dissolves in water to form bases
What are the characteristics of a nonmetal oxide
Simple covalent molecules that dissolve in water to form acids
In what ratio does halides bond with group 1 elements
1:1
In what ratio does halides bond with group 2 elements
1:2
In what ratio does halides bond with group 13 elements
1:3
In what ratio does halides bond with group 14 elements
1:4
In what ratio does halides bond with group 15 elements
1:3
In what ratio does halides bond with group 16 elements
1:2
In what ratio do halides bond with halides
1:1
What happens when halides form with metals
They form ionic solids
What happens when halides bond with non metals
They form simple covalent molecules
What do halides end with when bonding
They end with ide
