Unit 2 Flashcards
Chemical symbol
Abbreviation of the elements
atomic number
indicates # of protons, or electrons
Must be equal to have a stable element
Atomic mass
indicates # protons plus # Neutrons
the reason its not a whole number is because of isotopes
AMU
Atomic Mass Unit(dalton)
Matter
can be described using physical and chemical properties.
Mixtures
2 or more substances mixed together, but not clearly chemical combined
heterogenegus
consists of 2 or more clearly distinct items which can separate (trail mix
homogenegus
consists of 2 or more items which appear uniform (ex. milk)
elements
pure substances made of atoms that cant be broken down, made up of subatomic particles
CHONPS
6 of of the 92 elements make up 96% of all living organisms on earth
Octant rule
All orbitals other then the first have 8 electrons on them
What makes up the other 4% of living organisms
Ca, P, K, S, Na, Cl, Mg, and the trace elements make up the other 4% of an organisms weight
Trace elements
what can happen if you have a deficiency in the trace elements?
you will be sick
lack of iron
anemia
lack of iodine
goiter and hypothyroidism
Diatomic Elements
Always found paired together in nature (H2, N2, O2, F2, Cl2, Br2, I2)
Isotopes
elements with same # protons and electrons, but different # neutrons in the nucleus
What makes a isotope unstable or radioactive
If protons and neutrons differ a lot
When the nucleus breaks down what does it give off?
particles and energy
What do radioactive isotopes cause
change in DNA
what electrons are involved in chemical reactions
valence electrons
what happens when two incomplete outer shell atoms react
They give up or acquires electrons so the two atoms end up with complete outer shells
covalent bonds
involves a sharing of electrons between 2 or more atoms
