Donna Varamo
September 1, 2016
LO 1: Define basic terms regarding matter and list the properties of the 3 major subatomic particles
Matter- anything that takes up space and has mass
Energy- allows us to do work
o Cannot be created or destroyed
Element- a substance that cannot be broken down into other substances by chemical reactions
o Main elements of human body- O (65%), C (18%), H (9%), N (3%)
These are the elements in major compounds in the body
o Various trace elements
Magnesium is needed for enzymes to work
Phosphorus is in DNA/ribosomes
Atom- smallest unit of any elemental substance that still retains the properties of an element
o Proton: + charge, weight is 1 amu
o Neutron: neutral charge, weight is 1 amu
o Electron: - charge, weight is 1/2000 amu
Only things involved in chemical reactions
o Protons and neutrons are in nucleus, electrons outside the nucleus
Atomic number- # of protons
o Atomic number cannot be changed without changing the element
Atomic mass- # protons + # neutrons
o Can change in isotopes
Atomic weight- average weight of all isotopes
LO 2: Describe the use of radioactive isotopes in research and medicine
Isotope- neutrons vary but protons stay the same
Radioactive isotopes- unstable and release energy
?? at what temperature do cells grow the fastest??
o Experiment- radioactive material is absorbed by cells as nutrients, making cells radioactive
o Radioactive cells are divided into groups and each group of cells are put into different temperature
environments for a few days
o Cells are then put into a scintillation center→ will measure the flashes of light per minute per grou
o The group with the most flashes had the most growth
Most growth is at 37 degrees C
Oxygen can be made radioactive and injected into a person
o Will lighten where there is excessive oxygen use/activity
May be indicative of cancer or other disorders
o Observed via PET scan
Different isotopes can identify different problems
Body will either metabolize or excrete radioactive materials but some may persist longer than others
Radiometric dating- determines age of fossils
o Scientists measure the ratio of different isotopes and measure how many half lives have passed
since the organism died
, LO 3: Differentiate between results and conclusions
Results- verifiable data, observed directly
Conclusions- interpretation of results, what they might mean
Conclusions may be wrong and based on opinion, results are concrete
LO 4: How does an atom’s electron configuration determine its reactivity
Electron shells- one or more electrons at a given distance from the nucleus
o First shell- 2 electrons
o Outer shells- up to 8 electrons
o More energy at outer shells, electrons want to be at lowest electron shells so they fill in first
o Pairs of electrons represent orbitals
Orbitals- 3D space in which electrons exist 90-95% of the time
o Objects in nature tend to exist at their lowest energy state
o Lower energy shells- lower energy
o Valence shells- outer shell with possible unpaired electrons that are reactive
Absorbing energy- electron moves to shell farther from nucleus
Releasing energy- electron moves to shell closer to nucleus
Atoms with unpaired electrons are highly reactive (high energy low stability)
pairing of electrons decreases reactivity and increases stability→ less reactive
LO 5: Define covalent bonds and explain how electronegativity determines of the bond is polar or nonpolar
Covalent bond: electrons shared between 2 atoms→ both shells become full and a molecule is create
LO 6: Determine whether a covalent bond is polar or nonpolar
polar- unequal sharing of electrons
nonpolar- equal sharing of electrons
electronegativity- the ability of an atom to draw electrons to itself
same elements have same electronegativity→ nonpolar
partial charges used for polar bonds→ more electronegative→ δ- charge
allows interactions between molecules
LO 7: Define and illustrate hydrogen bonds
hydrogen bonds- attraction between δ+ H and an atom that is significantly more electronegative
LO 8: Describe and draw ionic bonds
ionic bond- an attraction between oppositely charged atoms
September 1, 2016
LO 1: Define basic terms regarding matter and list the properties of the 3 major subatomic particles
Matter- anything that takes up space and has mass
Energy- allows us to do work
o Cannot be created or destroyed
Element- a substance that cannot be broken down into other substances by chemical reactions
o Main elements of human body- O (65%), C (18%), H (9%), N (3%)
These are the elements in major compounds in the body
o Various trace elements
Magnesium is needed for enzymes to work
Phosphorus is in DNA/ribosomes
Atom- smallest unit of any elemental substance that still retains the properties of an element
o Proton: + charge, weight is 1 amu
o Neutron: neutral charge, weight is 1 amu
o Electron: - charge, weight is 1/2000 amu
Only things involved in chemical reactions
o Protons and neutrons are in nucleus, electrons outside the nucleus
Atomic number- # of protons
o Atomic number cannot be changed without changing the element
Atomic mass- # protons + # neutrons
o Can change in isotopes
Atomic weight- average weight of all isotopes
LO 2: Describe the use of radioactive isotopes in research and medicine
Isotope- neutrons vary but protons stay the same
Radioactive isotopes- unstable and release energy
?? at what temperature do cells grow the fastest??
o Experiment- radioactive material is absorbed by cells as nutrients, making cells radioactive
o Radioactive cells are divided into groups and each group of cells are put into different temperature
environments for a few days
o Cells are then put into a scintillation center→ will measure the flashes of light per minute per grou
o The group with the most flashes had the most growth
Most growth is at 37 degrees C
Oxygen can be made radioactive and injected into a person
o Will lighten where there is excessive oxygen use/activity
May be indicative of cancer or other disorders
o Observed via PET scan
Different isotopes can identify different problems
Body will either metabolize or excrete radioactive materials but some may persist longer than others
Radiometric dating- determines age of fossils
o Scientists measure the ratio of different isotopes and measure how many half lives have passed
since the organism died
, LO 3: Differentiate between results and conclusions
Results- verifiable data, observed directly
Conclusions- interpretation of results, what they might mean
Conclusions may be wrong and based on opinion, results are concrete
LO 4: How does an atom’s electron configuration determine its reactivity
Electron shells- one or more electrons at a given distance from the nucleus
o First shell- 2 electrons
o Outer shells- up to 8 electrons
o More energy at outer shells, electrons want to be at lowest electron shells so they fill in first
o Pairs of electrons represent orbitals
Orbitals- 3D space in which electrons exist 90-95% of the time
o Objects in nature tend to exist at their lowest energy state
o Lower energy shells- lower energy
o Valence shells- outer shell with possible unpaired electrons that are reactive
Absorbing energy- electron moves to shell farther from nucleus
Releasing energy- electron moves to shell closer to nucleus
Atoms with unpaired electrons are highly reactive (high energy low stability)
pairing of electrons decreases reactivity and increases stability→ less reactive
LO 5: Define covalent bonds and explain how electronegativity determines of the bond is polar or nonpolar
Covalent bond: electrons shared between 2 atoms→ both shells become full and a molecule is create
LO 6: Determine whether a covalent bond is polar or nonpolar
polar- unequal sharing of electrons
nonpolar- equal sharing of electrons
electronegativity- the ability of an atom to draw electrons to itself
same elements have same electronegativity→ nonpolar
partial charges used for polar bonds→ more electronegative→ δ- charge
allows interactions between molecules
LO 7: Define and illustrate hydrogen bonds
hydrogen bonds- attraction between δ+ H and an atom that is significantly more electronegative
LO 8: Describe and draw ionic bonds
ionic bond- an attraction between oppositely charged atoms
