Week One (Chemistry Basics) Flashcards
Chemistry is the study of _____ and the changes it undergoes
Physics is the study of ______, ______, and ______
Inorganic compounds contain all elements except _______
Organic compounds contain _______
Matter
Motion, Matter, Energy
Carbon
Carbon
Atoms
______ and ______ are inside the nucleus
_______ are outside the nucleus
______ are positively charged
______ are neutral
______ are negatively charged
Protons, Neutrons
Electrons
Protons
Neutrons
Electrons
_____ are the basic building blocks of matter
_____ are the smallest particle of an element that can enter into a ______ reaction
Atoms are composed of ______, ______, and ______
Atoms
Atoms, Chemical
Protons, Neutrons, Electrons
______ are comprised of a single kind of atom
An ______ is defined by its number of _______ (Z)
Protons have a mass of ______ = _______
Elements
Element, Protons
1 amu= 1.66 x 10-27th (power) kg
______ are comprised of more than one kind of atom in a fixed ratio by mass
______ are groups of atoms chemically bonded together into a discrete unit
Molecules are electrically _____
A ______ is matter that has a definite composition and constant properties
Compounds
Molecules
Neutral
Substance
_____ are atoms that have gained or lost electrons from their natural composition
Positive ion is a _____
Negative ion is a _____
Ions
Cation
Anion
______ cannot be broken down or decomposed into simpler substances by chemical or physical means, wheras ______ can be broken down into elements by chemical processes
_____ is both a molecule and and element
Elements
Compounds
O2 (Oxygen)
______ properties are characteristics that describe the chemical reactivity of a substance
Chemical reactions result in formation of ______ compounds
______ properties do not describe the chemical reactivity of a substance
A substance can display physical properties ______ a change in composition
Chemical
Different
Physical
Without
The ____ ____ (Z) of an element is the number of _____ in the nucleus. This determines the ____ of the atom
The _____ ____ (A) of an atom is the sum of the _____ number and the ______ number
The _____ _____ (or atomic weight) is the average mass of an atom in a natural sample of the element
Atomic Number, Protons, Identity
Mass Number, Proton, Neutron
Atomic Mass
_____ _____equal to the number of protons within a nucleus. Ex: AN of Carbon is __
Atomic number also tells the number of _____
_____ are weightless and are not used to calculate mass number
_____ _____ is the average of the mass numbers of all isotopes of an element
Atomic Number; 6
Electrons
Electrons
Atomic Weight (AKA: Atomic Mass)
_____ are atoms with the _____ atomic numbers but with _____ atomic weights (PP slide 13)
They have the _____ number of protons and electrons but a ______ different number of neutrons
____________ are heavier, unstable isotopes of an element that spontaneously decopose into more stable forms
____-____ is the time required to lose 1/2 of radioactivity
Isotopes, Same, Different
Same, Different
Radioisotopes
Half-Life
_____ ________ is used to determine mass of an atom or molecule (PP slide 12)
Isotopes have the ____ atomic number (Z) but ____ mass numbers (A)
In other words, same number of _____, but different number of ______
Mass Spectrometer
Same, Different
Protons, Neutrons
Dalton proposed three hypotheses to explain the ____ of ________ of _____ and _____ proportions
Laws of Conservation of Mass and Definite Proportions
Dalton’s Theory
1.) Each ______. is composed of tiny, indivisible particles called _____, which are ______ for that element but are ______ from atoms of other elements
Element
Atoms
Identical
Different
Dalton’s Theory
2.) _____ combination is simply the bonding of a definite, small whole number of _____ of each of the combining elements in a _____ ratio to make one ______ of the formed compound
A given compound always has the same ______ numbers and types of _____
Chemical, Atoms, Fixed, Molecule
Relative, Atoms
Dalton’s Theory
3.) No _____ are gained, lost, or changed in identity during a ______ reaction; they are just ______ to produce new substances
Atoms, Chemical, Rearranged
Law of Conservation of Mass
No _____ change in the total mass occurs during a _____ reaction
Detectable, Chemical
Law of Definite Proportions
Different samples of a ____ ______ always contain the same _____ in the same proportion by mass
Example: Water always contains ___% hydrogen and ____% oxygen
Dalton’s theory is significantly modified after the discovery of ______
Pure Compound
11.2%, 88.8%
Isotopes
Dmitri Mendeleev
Scientist who constructed the periodic table of elements, emphasizing that _____ and _____ properties are repeated in a ______ way
Chemical, Physical
Predictable
Periodic Table
The rows are called _____ and increase by _____ _____
The columns are called _____ or families, and the elements within a family have similar _____ and _____ properties
Periods, Atomic Number
Groups
Chemical, Physical
Periodic Law
The ______ of elements are periodic functions of their ______ ______
(AN/AW example on PP slide 22)
Properties, Atomic Number
Metals, Nonmetals, and Metalloids
Review Table on PP slides 23-24
Review Table on PP slide 23-24
Solids, Liquids, and Gases
Review Table on PP slide 25
Review Table on PP slide 25
Representative, Transition, and Inner Transition Elements
Review Table on PP slide 26
Review Table on PP slide 26
No ______ bonding takes place in ______
Most mixtures can be ______ by physical means
Mixtures can be _______ or _______
_______ cannot be separated by physical means, but only by _______ means
All compounds are ________
(Review PP slide 27)
Chemical, Mixtures
Separated
Heterogenous or Homogenous
Compounds, Chemical
Homogenous
Common Elements in Human Body and Important Functions
Major (96.1%)
Oxygen (O) - 65% body mass
Carbon (C) - 18.5% body mass
Hydrogen (H) - 9.5% body mass
Nitrogen (N) - 3.2% body mass
(O) - Component of organic and inorganic molecules. Needed for production of cellular energy (ATP)
(C) - Component of all organic molecules (carbs, lipids, fats, proteins, and nucleic acids)
(H) - Component of all organic molecules. As an ion, it influences the pH of body fluids
(N) - A component of proteins and nucleic acids (genetic material)
Common Elements in Human Body and Important Functions
Lesser (3.9%)
Calcium (Ca) - 1.5% body mass
Phosphorus (P) - 1.0% body mass
Potassium (K) - 0.4% body mass
Sulfur (S) - 0.3% body mass
(Ca) - Found as a salt in bones and teeth. Ionic form is required for muscle contraction, conduction of nerve impulses, and blood clotting
(P) - Part of calcium phosphate salts in bones and teeth. Also present in nucleic acids and part of ATP
(K) - Its ion is the major cation in cells. Necessary for conduction of nerve impulses and muscle contraction
(S) - A component of proteins, particularly muscle proteins
Common Elements in Human Body and Important Functions
Lesser (3.9%)
Sodium (Na) - 0.2% body mass
Chlorine (Cl) - 0.2% body mass
Magnesium (Mg) - 0.1% body mass
Iodine (I) - 0.1% body mass
Iron (Fe) - 0.1% body mass
(Na) - Major cation found in ECF. Important for water balance, nerve impulse conduction, and muscle contraction
(Cl) - Its negative ion is the most abundant anion in ECF
(Mg) - Present in bone, Also an important cofactor in number of metabolic reactions
(I) - Needed to make functional thyroid hormones
(Fe) - Component of Hgb (which transports O2 within RBCs. Also a component of some enzymes
Molecular Substances
A _____ is a group of substances chemically bonded together in a _____ unit
The _____ _____ of a substance gives the number of each kind of _____ in the molecule
Compounds composed of ______ tend to be molecular
Think: Covalent = _____ on the periodic table
Molecule, Discrete
Molecular Formula, Atom
Nonmetals, Close
Some Common Elements
Review PP slides 35-38
.
Iron
Fe++ (Ferrous) and Fe+++ (Ferric) forms
Iron is vital for the transport of ____ in Hgb
Which form of Iron is preferred and why?
O2 (Oxygen)
Fe++ (Ferrous) is the preferred form of Iron because it has a better O2 carrying capacity in comparison to Fe+++ (Ferric)
Methemoglobinemia
Causes and Treatment?
Met-Hgb is a type of hemoglobin that is in the Fe+++ (Ferric) state and it cannot bind oxygen
Causes may be environmental, genetic, or induced from pharmaceutical compounds
Methemoglobinemia
Causes and Treatment?
Children and pregnant women at high risk for exposure to high levels of Nitrites in drinking water
Cytochrome b5 reductase deficiency, G6PD deficiency, pyruvate kinase deficiency
Local anesthetic agents [Prilocaine and Benzocaine]
Prolonged Nipride administration, also quinones and sulfonamides
Tx: Methylene Blue (primary) and Ascorbic Acid (secondary)
What is the enzyme in the mitochondria that produces ATP?
Cytochrome Oxidase
Molecular Elements
(Think number at bottom right)
Diatomic:
Tetratomic:
Octatomic:
See also: ____ and _____
H2, N2, O2, F2, Cl2, Br2
P4
S8
Nitrous Oxide (N20) and Nitric Oxide (NO)
Ionic Compounds
Held together by ____ bonds, or the attraction of _____ charged ions
In the solid state, ionic compounds form ______ ______
_____ are attracted to all the neighboring _____, not just one. Thus, there are no ____ ionic “molecules”
Ionic, Oppositely
Crystalline Lattices
Cations, Anions, Discrete
Chemically Inert Elements
Inert elements have their outermost energy level ( ____ ____) fully occupied by electrons
Number of electrons to complete valence shell is __
Valence Electrons
8
Chemical Bonds
An energy relationship between the _____ of the reacting atoms
Electrons occupy regions of space called ____ ____ that surrounds the nucleus in layers
Each ____ holds a specific number of ____ and represents a different energy level
Electrons
Electron Shells
Shell, Electrons
Chemical Bonds
_____ are formed using the _____ in the outermost energy level
_____ shell: Outermost energy level containing chemically ____ electrons
_____ rule: Except for the first shell which is full with __ electrons, atoms interact in a manner to have ____ electrons in their valence shell
Bonds, Electrons
Valence, Active
Octet, 2, 8
Chemically Reactive Elements
Reactive elements have their outermost energy level fully occupied by __ electrons
8
Ionic Bonds
Chemical bonds that form between two atoms that ______ one or more electrons from one atom to the other
Ions are _____ particles
An _____ is an electron acceptor; carrying a net _____ charge due to the extra electron
A _____ is an electron donor; carrying a net ______ charge due to the loss of an electron
Transfer
Charged
Anion, Negative
Cation, Positive
Ionic Bonds
Ionic compounds form ______ instead of individual molecules
_____ are large structures of cations and anions held together by _____ bonds
Common example of ionic bond: (Hint: Salt crystal)
Crystals
Crystals, Ionic
NaCl
Covalent Bonds
Form when electrons are ______ between two atoms
Some atoms are capable of sharing two or three electrons between them, resulting in ____ or ____ covalent bonds
Electron sharing produces ______
Shared
Double or Triple
Molecules
Polar and Nonpolar Molecules
Electrons shared ______ between atoms produce ______ molecules
______ sharing of electrons produces ______ molecules
A _____ molecule has a net ______ as a result of the _______ charges (having a partial positive and partial negative charge)
______ is an example of a polar molecule with this slighty postiive and slightly negative charge
Equally, Nonpolar
Unequal, Polar
Polar, Dipole, Opposing
Water
Covalent Bonds
____ distribution of charges
Hydrogen atoms form ____ bonds
Oxygen atoms form ____ bonds
Nitrogen atoms form ____ bonds
Carbon atoms form ____ bonds
Equal
Single
Two
Three
Four
Hydrogen Bonds
Hydrogen bonds are ____ attractions that form between partially charged atoms found in _____ molecules
Common in dipoles, such as _____
H+ bonds are responsible for the _____ _____ of water
H+ bonds give the molecule a _____-_______ shape
H+ bonds tend to _____ the lung (reason surfactant is needed)
Weak, Polar
Water
Surface Tension
Three-Dimensional
Collapse
Ions
An ion is an atom or group of atoms with a ______
Cations are _____ charged ions. Cations are formed by ____ of electron. ______ tend to form cations.
Anions are ______ charged ions. Anions are formed by ____ of an electron. ______ tend to form anions.
For ______ cations, the ionic charge equals the group number (PP page 56)
Charge
Positive, Loss, Metals
Negative, Gain, Nonmetals
Representative
Ions
For representative anions, the ionic charge equals the _____ number minus __
To name monatomic anions, add the suffix ___ to the stem name
Ex: Cl, S2, N3, O2
Group, 8
“Ide”
Chloride ion, Sulfide ion, Nitride ion, Oxide ion
Naming Transition Metal Cations
The ____ charged ion is the “ous” ion and the ____ charged ion is the “ic” ion
Cr2 versus Cr3
Fe2 versus Fe3
Lower, Higher
Chromous ion versus Chromic ion
Ferrous ion versus Ferric ion
Naming Molecular Compounds
Molecular compounds are made up of ______ units (molecules) and usually consist of a small number of nonmetal atoms held together by ______ bonds
Molecular compounds with nonsystematic names?
Discrete, Covalent
Water, Ammonia, Methane, Ethane, Propane, Nitrous Oxide
Hydrates
Some ionic compounds incorporate a _____ number of _____ molecules into their formula unit
Naming hydrates only makes sense when you are dealing with _____ reagents
The number of _____ is indicated with a multiplier number
Examples: PP page 64
Fixed, Water
Solid
Waters
Desiccants
A desiccant is the _____ (dry compound) form of a compound that has a strong tendency to form a ______, and is used to ______ the last traces of water from a system
The most commonly used desiccant is _____ gel (SiO2)
Addition of water to a desiccant is a ______ process, so saturated desiccants can be used as _______
Anhydrous, Hydrate, Scavenge
Silica
Reversible, Moisturizers
