PM1B - Autumn - Structure and bonding Flashcards
(17 cards)
What does the Group Number in the periodic Table Represent
Group number in the period table means the amount of electrons in a valence shell.
Describe an atom including the valence shell
The valence shell is the outa shell ( Last Shell).
An atom has protons + neutrons+electrons.
Protons are +
Neutrons are neutral.
Electrons are negative -
Electrons are more involved in chemical bonding.
Periodic Table Overview
The Middle section in yellow isnt classed as being in a group
As we go down the table ( sideways) each atom gains a shell, therefore atomic radius and size increases.
As we go to the right, atomic radius decreases as we are moving within a shell and the proton increases by 1 so stronger electromagnectic attraction felt by the electrons and the radius shrinks. so atomic radius increases down and left.
What is Ionic Radius
Electrons repell each other so adding an electron makes an atom bigger. Ions with the same electronic configuration will have radius decrease as atomic number increases.
What is Ionization Energy
Energy required to remove an electron from an atom. The electromagnetic forces with attract the electron to the proton decrease with distance = so further away the electron is from the nucleus the easier it is to pull it away. so ionization energy trend increases up and right.
What Is Electronic Affinity
Electronic affinity - How much an atom wants to gain an electron. Also up and right on the periodic table but this does not include the noble gases in group 8 as their shells are already full. The elements on the left, they dont want to gain electrons they would rather lose them.
Describe Electronegativity
This is the abilty for an atom to hold an electron tightly. This trend is also up and right. For example flourine, holds its electrons best as it has more protons for its energy levels. (protons are in the nucleus and because they are positive will attract electrons because they are negative)
What is the Atomic Weight and Atomic Number
The atomic weight is the sum of protons plus neutrons
Number of protons = Atomic number
How do we find the number of protons / Neutrons and Electrons
Number of protons = Atomic number
Number of neutrons - Subtract atomic number from mass number
Electrons = Number of protons/Atomic number.
Discuss electron shells and orbitals
- Each shell has different orbitals
- An orbital is an area where there is a high probability of finding an electron
- Different orbital shapes are possible ( S,P,D,F)
- Outermost electrons are called valence
- 1st shell can hold 2
- 2nd shell can hold 8
- 3rd shell can hold 18
S oribals normally hold 2
P orbitals can hold 6
Dorbitals normally 10
Describe the Shapes of the orbitals
s orbitals are normally sphere - can hold 2 electrons
P orbitals are dumbell shaped, normallly 3p orbitals that hold 2 electrons each. ( 6 in total)
The Principles of arranging electrons
- The Orbitals of lowest energy are filled first ( Aufbau principle)
- Only 2 electrons can occupy the same orbital ( Pauli exclusion principle )
- If 2 or more empty degenerate orbitals are available, one electron is placed in each until they are all half full ( Hunds rule)
How does an Atom become an ION
Normally with Ions if we lose an electron for example, sodium has 11 protons and 11 electrons, but if we lose an electron we would have 11 protons and 10 electrons. This would make the overall charge +1, and therefore the sodium atom will become a sodium ION.
Adding an electron here would make it a negative charge, as electrons are negative.
Draw the Functional group Alcohol
Alcohol has an OH group
Draw the functional Group Ether
Ether is an Oxygen bonded to 2 different carbon atoms
Draw the functional group Amine
Amine is a nitrogen bonded to 2 Hydrogen atoms ( can have primary, secondry and tertiary )
Draw the functional group Alkyl Halide
Alkyl halide consists of an Halogen ( F, CL, BR ) also known as halogenoalkanes
