Topic 1 - The Periodic Table Flashcards
What is the mass number?
The number of the protons and neutrons.
Bigger
What is the atomic number?
The number of protons and (electrons).
Smaller
What is the charge of a proton?
+1
What is the mass of a proton?
1
What is the charge of a neutron?
0
What is the mass of a neutron?
1
What is the charge of an electron?
-1
What is the mass of an electron?
Negligible
What is the definition of ions?
Electrically charged particles formed when atoms lose or gain electrons. They have a different number of electrons and protons.
What is the definition of an isotope?
Atoms of an element with the same number of protons but a different number of neutrons. This means their mass numbers will be different but atomic number will be the same.
What is relative atomic mass?
The mean mass of an atom of an element relevant the mass of an atom of carbon-12.
What is the equation for relative atomic mass?
(Abundance X mass) + (Abundance X mass) / 100
What is the definition of electron configuration?
How electrons are arranged in the shells.
How many electrons can each shell hold?
Shell 1 - 2
Shell 2 - 8
Shell 3 - 8
Shell 4 - 2
2.8.8.2
What does the group number tell you?
The number of electrons in the outer shell.
It has elements with similar chemical properties.
What does the period number tell you?
The number of shells.
What did John Dalton discover about the atom?
Atoms are spheres (had a particular size and mass)
Billiard ball model
What did JJ Tomson discover about the atom?
Discovered the electron negatively charged particles dotted in the sphere.
Plum pudding model
What did Rutherford discover about the atom?
Positive nucleus with electrons around the outside.
Empty space between nucleus and electrons.
Nuclear model
What did Niels Bohr discover about the atom?
Electrons orbit the nucleus in shells.
What is an atom?
The smallest particle of an element that still has its chemical properties.
What is a molecule?
Two or more atoms chemically joined together.
What is a compound?
Two or more different elements chemically joined together.
Similarities between Modern periodic table and Mendeleev’s periodic table.
• Elements into groups/periods
• Metals and non-metals
• Elements with similar properties in same group.
Differences between modern periodic table and Mendeleev’s periodic table.
• No gaps in modern periodic gable.
• Different element names
• More elements in modern
• Accurate atomic mass in modern
• Groupings aren’t the same
• Mendeleev’s table arranged by relative atomic mass but now it’s atomic number.
• Mendeleev’s didn’t include noble gasses (group 0)
What side are metals on the periodic table?
Left
What side are non-metals on the periodic table?
Right
What is the charge when electrons are gained?
Negative charge
What is the charge when electrons are lost?
Positive charge
How did Mendeleev arrange the elements?
In order of increasing relative atomic mass.
However this wasn’t always true because of the relative abundance of isotopes of some pairs of elements.
What is the difference in the atomic structure of metals and non-metals?
• Metal elements give away electrons in their reactions to form positive ions.
• Non-metal elements gain electrons in some of their reactions to form negative ions.
