Unit 1 Chem - A1 structure and bonding in applications in science Flashcards
What does the nucleus contain?
Positive Protons and Neutral neutrons
What surrounds the nucleus
Energy shells
What do the energy shells contain?
Negative electrons
Relative mass of protons and neutrons
1
Relative mass of an electron
0
Maximum no of electrons in shell 1
2 electrons
Maximum no of electrons in shell 2
8
Maximum no of electrons in shell 3
18
Maximum no of electrons in shell 4
32
Maximum no of electrons in shell 5
50
What are the energy levels/shells broken down into (sub shells) ?
S,p,d,f orbitals
Aufbau principal
Electrons fill the orbital with the lowest available energy state in relaxation to the proximity to the nucleus before filling orbitals with higher energy states.
What’s the point of Aufbau principle
It gives the most stable electron configuration possible
Electrons have the same charge so they _________ each other
Repel
Orbitals
Regions where there is a 95% probability of locating an electron. An orbital can hold a maximum of two electrons.
Electronic Configuration
The distribution of electrons in an atom or molecule
Spin
Electrons have two possible states, spin up or down. In each orbital an electron will be in a differ spin state.
Bohrs theory
An electrons shells orbit in circles around the nucleus
How many electrons can s block hold
2
How many electrons can p block hold?
6
How many electrons can d block hold?
10
How many electrons can f block hold?
14
Ionic bonding
Atoms transfer electrons to achieve a full outer shell
And is the strong electrostatic attraction between oppositely charged ions
When does ionic Bonding occur
Between metals and non metals
Do the non metals in ionic bonding lose or gain electrons?o
Gain
Do metals in ionic bonding lose or gain electrons?
Lose
An Atom that that loses an electron becomes a positively charged _____
Cation
An Atom that gains electrons becomes a negatively charged _________
Anion
Ion
Atom that loses or gains an electron
Atom
The smallest part of a substance which cannot be broken down chemically
When atom loses an electron it g________
Gains
When an atom gains an electron it l_____
Loses
Two factors that affect charge density
Ionic charge
Ionic radius
Group 1,2,3 metals will donate electrons to become?
Cations
1+ cation
2+ cation
3+ cation
How is a -2 anion more attractive than a -1 anion?
It’s smaller in size and larger in charge so the charge is more concentrated and this makes it more attractive
Ionic charge
Atom/ ion with a net electrical charge
Charge density increases as _______ decreases.
Radius
As you move down a group the atomic radius _________ because there is an extra _______ due to more electrons
Increases
Shell
How is the strength of a ionic bond measured?
Electrostatic force between two oppositely charged ions
The bigger the ionic charge results in a stronger a_______ and stronger ionic _____
Attraction
Bond
electrostatic attraction
the force experienced by oppositely charged particles which hold them strongly together
giant ionic lattice
a regular arrangement of positive and negative ions
