Week One (Chemistry Basics) Flashcards by Lindsay Reynolds

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

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Atoms

______ and ______ are inside the nucleus

_______ are outside the nucleus

______ are positively charged

______ are neutral

______ are negatively charged

Protons, Neutrons

Electrons

Protons

Neutrons

Electrons

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_____ 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

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______ 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

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______ 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

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_____ are atoms that have gained or lost electrons from their natural composition

Positive ion is a _____

Negative ion is a _____

Ions

Cation

Anion

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______ 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)

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______ 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

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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

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_____ _____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

Atomic Weight (AKA: Atomic Mass)

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_____ 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

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_____ ________ 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

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Dalton proposed three hypotheses to explain the ____ of ________ of _____ and _____ proportions

Laws of Conservation of Mass and Definite Proportions

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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

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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

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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

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Law of Conservation of Mass

No _____ change in the total mass occurs during a _____ reaction

Detectable, Chemical

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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

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Dmitri Mendeleev

Scientist who constructed the periodic table of elements, emphasizing that _____ and _____ properties are repeated in a ______ way

Chemical, Physical

Predictable

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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

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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

Representative, Transition, and Inner Transition Elements

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

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

## Footnote 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)

## Footnote 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 \_\_\_\_\_\_

## Footnote 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

## Footnote 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)

## Footnote 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)

## Footnote 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

## Footnote 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

## Footnote 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?

## Footnote 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

## Footnote 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 \_\_\_\_\_\_\_

## Footnote Anhydrous, Hydrate, Scavenge Silica Reversible, Moisturizers