Exam 1 Flashcards
Designed to mimic the bodys natural release profile
Humalog
Clusters of 6 insulin molecules
Hexamers
The scientific method
Observations, hypothesis, experiments, theory
Recording qualitative or quantitative data
Observations
Explanation of observations
Hypothesis
Change one variable at a time, test hypothesis
Experiments
Explains experiment, predicts further outsome
Theory
Amount of matter in an object
Mass
Measures the force with which gravity pulls on an object
Weight
How close to the true value a given measurement is
Accuracy
How well a number of independent measurements agree with each other
Precision
Total numner of digits recorded for a measurement
Significant figures
Method that uses a conversion factor to convert a quantity expressed in one unit to an equivalent quantity in a different unit
Dimensional analysis
Expresses the relationship between two different units
Conversion factor
Independent of sample size, temperature and melting point
Intensive properties
Dependent on sample size, length and volume
Extensive properties
Characteristics that DO NOT involve a change in a sample’s chemical makeup
Physical properties
Characteristics that DO involve a change in a sample’s chemical makeup
Chemical properties
Left side of zig zag line except for hydrogen
Metals
Right side of zig zag line
Nonmetals
Lie along zig zag line
Semimetals, metalloids
Mass is neither created nor destroyed in chemical reactions
Law of conservation of mass
Different samples of a pure chemical substance always contain the same proportion of elements by mass
Law of definite proportions
Elements can combin in different ways to form different substances, whose mass ratios are small whole-number multiples of each other
Law of multiple proportions
Elements are made up of tiny particles called
Atoms
Negatively charged particles
Electrons
Mainly empty space with the mass concentrated in a tiny central hole
Nucleus
Number of protons in an atoms nucleus. Equivalent to the number of electrons around an atoms nucleus
Atomic number
Sum of the number of protons and the number of neutrons in an atoms nucleus
Mass number
Atoms with identical atomic numbers but different mass numbers
Isotopes
Weighted average of the isotopic masses of the elements naturally occurring isotopes
Atomic mass
Mass in grams of one mole of any element. Numerically equivalent to its atomic mass
Molar mass
Results when two atoms share several (usually 2) electrons. Typically nonmetal bonded to nonmetal
Covalent bond
Unit of matter that results when two or more atoms are joined by covalent bonds
Molecule
Transfer of one or more electons from one atom to another. Strong electrical attraction between charged particles. Typically metal bonded to nonmetal
Ionic bond
Charged particle
Ion
Positively charged particle.
Cation
Negitively charged particle
Anion
Neutral compond in which the total number of positive charges must equal the total number of negative charges
Ionic compound
Helium-4 nucleus
Alpha particle
An electron
Beta particle
High-energy photon
Gamma particle
Has the same mass as an electron but the opposite charge
Positron
Process in which the nucleus captures an inner-shell electron, thereby converting a proton to a neutron
Electron capture
Loss in mass that occurs when protons an neutrons combine to form a nucleus. Loss in mass is converted into energy that is released during the nuclear reaction and is thus a direct measure of the binding energy holding the nucleus together
Mass defect
Self-sustaining reaction whose product initiates further reaction
Chain reaction
