Ch 2 pt 1 Flashcards
What is matter?
Has mass and occupies space
Forms of matter
Solid, liquid, gas
Example of solid
Bone
Example of liquid
Blood
Example of gas
Oxygen
What is atom?
Basic unit of an element; smallest particle
What is the symbol O?
Oxygen
What is the symbol C?
Carbon
What is the symbol H?
Hydrogen
What is the symbol N?
Nitrogen
What is the symbol Ca?
Calcium
What is the symbol P?
Phosphorus
What is the symbol S?
Sulfur
What is the symbol K?
Potassium
What is the symbol Na?
Sodium
What is the symbol Cl?
Chlorine
What is the symbol Fe?
Iron
What is the symbol Mg?
Magnesium
Charge on Neutron
No charge
Charge on Proton
Positive charge
Charge on Electron
Negative charge
Proton number=
Atomic number
Neutron number=
Atomic mass - atomic number
Electron number=
Proton number
Isotopes
Are different atoms of the same element
Isotopes have the same number of what?
Protons and electrons
Isotopes have different what?
Atomic masses
Isotopes have the identical what?
Chemical characteristics
Physical half-life
The time for 50% of radioisotope to become stable
Radioisotopes
Same chemical element with different masses; excess neutrons so unstable
What is a valence shell?
Organized into columns based on number electrons in outer shell.
Biological half-life
The time required for half of the radioactive material from a test to eliminated from the body
Octet rule
Elements tend to lose, gain, or share electrons to obtain complete outer shells with eight electrons
What are ionic bonds?
Ionic compounds are structures composed of ions held together in a lattice
Ions
Atom with a pos. or neg. charge and loss or gain an electron
Lose a e-
Cation
Give/take e-
Ionic
Gain a e-
Anion
Cation are ions with a
Positive charge
Anions are ions with a
Negative charge
Cations and anions bound by
Electrostatic forces
Covalently bonded molecule
Electrons shared between atoms of two or more different elements.
Molecular and structural formula
Indicates number and types of atoms
What are isomers?
Same chemical formula but different structure
C6 H12 O6
Glucose, fructose, galactose
Formed commonly in human body using
Carbon, hydrogen, oxygen, nitrogen (CHON)
Single covalent bond
One pair of electrons shared (2 layers)
Double covalent bond
Two pair of electrons shared (4 layers)
Triple covalent bond
3 pair of electrons shared (6 layers)
How many electrons does carbon need to satisfy octet rule?
4
Electronegativity
Relative attraction of each atom for electrons
Nonpolar covalent bond
Two atoms of same element have equal attraction for electrons
Polar covalent bond
Sharing of electrons unequally
More electronegative atom develops a partial
Negative charge
Less electronegative atom develops a partial
Positive charge
Amphipathic molecules
Large molecules with polar and nonpolar regions
