Unit 3 (Atomic Structure) Flashcards
Explain the properties of subatomic particles. Symbol charge and relative mass
- proton
- neutron
- electron
Proton - p+, +1, 1
Neutron - n^o, 0, 1
Electron - e-, -1, 1/1840
Explain where the subatomic particles are located
- protons
- neutrons
- electrons
- Protons - in the nucleus
- Neutrons - in the nucleus
- Electrons - in the electron cloud outside the nucleus in energy levels (also in the nucleus??)
- Electrons and protons attract each other like positive and negative btw
Explain what the atomic number is
- the definition
- what it always is
- examples
- a connection and how it relates to elements
- what it means for neutral elements with no charge
- The number of protons in an element
- It is always a whole number
- Oxygen has an atomic number of 8, so there are 8 protons in the nucleus.
- It will never change for an element and connects to social security numbers. It identifies it.
- Neutral elements (no charge) have same # of protons and electrons
Explain what the atomic mass is
- where it is read off of
- what the number will always be
- what it is
- It is read off the periodic table.
- The number will have a decimal.
- It is the weighted average of all the elements isotopes.
Explain mass numbers
- what it is
- what it always will be
- how to find the number of neutrons
- Number of protons and neutrons combined
- It is always a whole number
- neutrons = mass # - atomic # Example: Oxygen’s mass number is 16 and its atomic number is 8. The number of neutrons will be 16-8 = 8.
Explain what isotopes are
- what they actually are
- what are they chemically
- what they always have
- how they are written
- examples
- Atoms with the same number of protons, but different number of neutrons
- They are chemically alike
- Have different written mass numbers
- Written like this: Element Name - Mass Number
- Examples: Neutral hydrogen isotopes
Explain what an ion is
- what it is
- how it forms
- An atom or group of atoms that has a positive or negative charge
- Forms when an atom gains or loses electrons
Explain how to write ions
- how to write the charge
- how to write the electrons lost
- An ionic charge is written as a sign (positive “+” or negative “-”) followed by a number
- The number represents the amount of electrons gained or lost.
Explain what cations are
- how they are formed
- definition
- what changes, and what stays the same
- examples
- Metals lose electrons to become cations.
- An atom or group of atoms with a positive charge
- Have the same name as the element that forms them, but different chemical properties
- Examples: Sodium and Calcium Na+1 = sodium cation, Ca+2 = calcium cation
Explain Anions
- what they are
- what the name of them are
- how they form
- what are examples
- Atoms or groups of atoms with a negative charge
- The name of the anion is the element name with “-ide” on the end
- Nonmetals tend to form ions by gaining electrons
- Examples: Oxygen and Chlorine O-2 = Oxide anion, Cl-1 = chloride anion
There’s also information about abbreviating ions but I don’t think it’s that important??
Atomic Mass Units (amu)
- what they are defined as
- what is it. Like what does it measure
Defined as 1/12 the mass of a Carbon-12 atom.
This is the way in which atomic mass is measured on the Periodic Table
Abbreviated “amu”
carbon - atomic number 6. Atomic mass 12.01
What are the 3 things you need to find the atomic mass. kinda only 2 for the calculation but still
Number of stable isotopes
mass of each isotope
natural % abundance of each isotope
Percentages must equal 100.
Explain how to calculate atomic mass like a weighted average (remember the correct way to show work)
Also remember to label with amu units
atomic mass1 (%1/100) + atomic mass2 (%2/100) = atomic mass of the element
