Bonding

Created by

Jasmine Steele

Cards (42)

Describe the structure of an atom
A central positively charged nucleus containing protons and neutrons surrounded by orbiting electrons in shells
Relative mass of a proton
1
Relative mass of a neutron
1
Relative mass of an electron
1/1840
Relative charge of an electron
-1
Relative charge of a proton
+1
Relative charge of a neutron
0
What is the atomic number?
The atomic number is the number of protons in the nucleus of an atom
What is the mass number?
The mass number is the total number of protons and neutrons in the nucleus of an atom
What is an isotope?
Isotopes are atoms that have the same number of protons (so they are atoms of the same element), but they have a different number of neutrons (so they have a different mass number)
How is relative atomic mass calculated?
(mass number 1 x abundance) + (mass number 2 x abundance)
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total abundance
How many electrons can the third shell hold?
8 electrons
Why are noble gases unreactive?
They have a full outer shell of electrons
What is a compound?
A compound is a substance formed when two or more different elements are chemically combined
What is a cation? 
A positively charged ion
What is an anion?
A negatively charged ion
Why do atoms bond?
Atoms bond with other elements in order to obtain a noble gas (stable) electronic structure
How many elements exist naturally as single unbonded elements?
Only six elements exist naturally as single unbonded atoms. These monatomic elements are called the noble gases.
What is an ion?
A charged particle formed when an atom gains or loses electrons
What is a molecular ion?
A charged particle containing more than one atom
What is a cation? 
A positively charged ion
What is an anion?
A negatively charged ion
What type of elements form ionic bonds?
Ionic bonding occurs in compounds that contain a metal and a non-metal, usually a compound of a Group 1 or 2 element, with a Group 6 or 7 element. The atoms of these elements do not have filled outer shells and need to bond to obtain a full outer shell and become stable.
What happens when an ionic bond is formed between two atoms?
-Electrons are transferred from the metal atom to the non-metal atom.
-Oppositely charged ions are formed - the metal ion has a positive charge, the non-metal ion has a negative charge - and the ions are held together by the attraction between opposite charges - this is the ionic bond. An ionic bond is the attraction between oppositely charged ions.
-Each ion formed has a filled outer shell, and hence a stable noble gas electronic structure.
What is an ionic bond?
the attraction between oppositely charged ions
are ionic bonds weak or strong?
Ionic bonds are strong and require substantial energy to break.
How are ionic bonds held together?
Ionic bonds are held together by the attraction between opposite charges
When is a covalent bond formed?
A covalent bond is formed when two atoms share electrons to obtain a noble gas configuration
What type of elements form covalent bonds?
Covalent bonding occurs between non-metals
Are covalent bonds strong or weak?
Covalent bonds are strong and require substantial energy to break.
What is a covalent bond?
A shared pair of electrons
What is a molecule? 
two or more atoms covalently bonded together
What are the atoms in molecules held together by?
covalent bonds
What does diatomic mean?
Diatomic means that there are two atoms covalently bonded in a molecule
What can a covalent bond be represented by in structural formulae?
a line (-)
What are the different types of covalent bonds?
single covalent bonds, double covalent bonds and triple covalent bond
What is a single covalent bond?
A bond formed when two atoms share a single pair of electrons. Represented by a single line (-)
What is a double covalent bond?
A bond formed when two atoms share two pairs of electrons. Represented by a double line (=)
What is a triple covalent bond?
A bond formed when two atoms share three pairs of electrons. Represented by a triple line.
What is metallic bonding?
The attraction between the positive ions in a regular lattice and the delocalised electrons.