Structure And Bonding Flashcards
What are the 3 states of matter and their symbols
Solid(s) liquid (l) gas (g) aqueous (aq)
Describe the process of melting,
Solid turns into a liquid due to the heating of atoms inside, causing them to gain energy and vibrate and move freely until it overcomes the attractive forces
Describe the process of boiling
Liquid turns into a gas
Heating causes particles to move faster and collide increasing the vapor pressure until the liquid boils and forms gas bubbles
Describr the process of condensing
When a gas cools and loses energy causing its molecules to slow down and change into a liquid
What is the process of evaporation
When a liquid turns into a gas
What is the process of deposition
When a gas turns into a solid
Why do different substances have different melting and boiling points
Because the intermolecular forces between particles vary:
for example metallic compounds have giant structures, meaning they need more energy to break their many strong bonds, compared to other compounds that may have a weak intermolecular force between particles and therefore little energy needed to break it
Describe the factors that affect rate of evapotation
Temperature
Surface area
Structure of liquid (weak or strong bonds)
Air movement
State the particles involved in ionic bonding
(Positive) Metals and (negative) non metals
State the particles involved in covalent bonding
Non metal compounds
State the particles involved in metallic bonding
Metallic compounds
What are the properties of group 1 elements
Highly reactive - as they have a single electron on their outer shell which can easily become a +1 ion.
Low M and B point that decreases - there small number of electrons mean they have a weak structure, as you go down the molecules get larger and bonds become weaker
Good Conductors - their valence electron can move easily through the structure and carry a charge, therefore conduct
Reactivity increases as you go down - the outer electron gets further from the nucleus as you go down and can be lost more easily.
What are the properties of group 7 element
Don’t conduct - as there non metals
Highly reactive - 1 electron short of a full outer shell
M/B points are high that increase - have strong intermolecular forces, as you go down the atoms increase in size, as they gain extra electron shell which requires more energy to break
Reactivity decreases - As you move down the group, the atomic size increases, meaning that the outer electron is further from the nucleus. This results in a weaker attraction between the nucleus and the outer electron, making it harder for the halogen to gain an electron.
What are the properties of the noble gases
Poor reactivity - full outer shell
M and B points increases due to atomic sizes
Don’t conduct - they are monatomic (exist as individual atoms) and have a full valence shell, therefore no electrons to carry a charge
Describe how a group 1 metal atom becomes a positive ion
A Group 1 metal atom becomes a positive ion by losing its single outer electron, resulting in a positive charge. Because it only had 1 electron on its outer shell, it now has a full shell, (even if its zero)
What is an ion
A atom or molecule that has gained or lost an electron
What is an iscotope
An atom of the same element with a different number of neutrons
Resulting in a different atomic mass
Explain how electron transfer allows ionic bonding to occur in the compound formed when a group 1 metal reacts with a group 7 metal
Group 1 metals lose an electron and the group 7 nonmetals gain an electron. Leaving
Group 1s a positive charge and 7s a negative charge. These oppositely charged ions attracted to each other because of the electrostatic force, forming an ionic bond
Explain the charge of a monatomic ion
The charge of a monatomic ion is determined by the number of electrons an atom gains or loses; if it loses electrons, it becomes a positively charged ion (cation), and if it gains electrons, it becomes a negatively charged ion (anion).
Describe how a group 7 non-metal atom becomes a negative ion
Group 7 non-metals require 1 more electron to fill their outer shell, resulting in a negative charge as there are more electrons than protons
Sublimation
When a solid turns into a gas
Why when say oxygen (6) reacts with sodium (1), why do we say oxygen is ‘reduced’ when it is the element that gains electrons?
Because its charge is reduced
