Chlorine is an element that consists of 17 protons, an average of 18.5 neutrons and 17 electrons. It has an atomic number of 17, and an average nuclear charge of 35.5. There are 2 isotopes of chlorine that are 35Cl and 37Cl. 35Cl has an atomic mass of 35 and a natural abundance of 75%. 37Cl has an atomic mass of 37 and a natural abundance of 25%. The average atomic mass or nuclear charge equates to 35.5. Both of the isotopes have the same atomic number. (BBC Bitesize. Atoms and the periodic table. 2014)
Gold: Au, Arsenic: As, Molybdenum: Mo, Barium: Ba, Lead: Pb, Niobium: Nb, Technetium: Tc,
Rhodium: Rh, Scandium: Sc
TASK 6
The periodic table distinguishes metals from nonmetals, as the metals are present on the left hand side of the …show more content…
The elements are arranged based on atomic numbers and electronic configurations. Groups of the periodic table indicate the number of valence electrons in an element’s atom. Periods of the periodic table indicate the total number of electron shells in an element’s …show more content…
There are metallic bonds between metals that affect their properties. Valence electrons from orbitals s and p delocalize to form a “sea” of electrons which makes up the metallic bond. All metals can conduct electricity to different extents. Electrical conductivity arises from the movement of electrons. Metals have valence electrons that are free to move about, therefore, electricity can be conducted due to these ‘free electrons’. Metals can usually conduct electricity faster than non-metals in a certain period of time and are known as good conductors of electricity. Metals also generally tend to have high melting and boiling points, this is because of the strong metallic bonds they have. The more delocalized electrons per atom, the stronger the bonding between them, thus the higher the melting and boiling point. Furthermore, due to the strength of the metallic bonds, metals are insoluble apart from in other liquid metals. (Sharon Keeley, Simon Little. 2003) (Boundless. Metallic Bonding
Gold: Au, Arsenic: As, Molybdenum: Mo, Barium: Ba, Lead: Pb, Niobium: Nb, Technetium: Tc,
Rhodium: Rh, Scandium: Sc
TASK 6
The periodic table distinguishes metals from nonmetals, as the metals are present on the left hand side of the …show more content…
The elements are arranged based on atomic numbers and electronic configurations. Groups of the periodic table indicate the number of valence electrons in an element’s atom. Periods of the periodic table indicate the total number of electron shells in an element’s …show more content…
There are metallic bonds between metals that affect their properties. Valence electrons from orbitals s and p delocalize to form a “sea” of electrons which makes up the metallic bond. All metals can conduct electricity to different extents. Electrical conductivity arises from the movement of electrons. Metals have valence electrons that are free to move about, therefore, electricity can be conducted due to these ‘free electrons’. Metals can usually conduct electricity faster than non-metals in a certain period of time and are known as good conductors of electricity. Metals also generally tend to have high melting and boiling points, this is because of the strong metallic bonds they have. The more delocalized electrons per atom, the stronger the bonding between them, thus the higher the melting and boiling point. Furthermore, due to the strength of the metallic bonds, metals are insoluble apart from in other liquid metals. (Sharon Keeley, Simon Little. 2003) (Boundless. Metallic Bonding