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Chemistry/Physics Test 1 > Week One (Chemistry Basics) > Flashcards

Week One (Chemistry Basics) Flashcards

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1
Q

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 _______

A

Matter

Motion, Matter, Energy

Carbon

Carbon

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2
Q

Atoms

______ and ______ are inside the nucleus

_______ are outside the nucleus

______ are positively charged

______ are neutral

______ are negatively charged

A

Protons, Neutrons

Electrons

Protons

Neutrons

Electrons

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3
Q

_____ 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 ______

A

Atoms

Atoms, Chemical

Protons, Neutrons, Electrons

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4
Q

______ are comprised of a single kind of atom

An ______ is defined by its number of _______ (Z)

Protons have a mass of ______ = _______

A

Elements

Element, Protons

1 amu= 1.66 x 10-27th (power) kg

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5
Q

______ 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

A

Compounds

Molecules

Neutral

Substance

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6
Q

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

Positive ion is a _____

Negative ion is a _____

A

Ions

Cation

Anion

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7
Q

______ 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

A

Elements

Compounds

O2 (Oxygen)

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8
Q

______ 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

A

Chemical

Different

Physical

Without

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9
Q

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

A

Atomic Number, Protons, Identity

Mass Number, Proton, Neutron

Atomic Mass

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10
Q

_____ _____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

A

Atomic Number; 6

Electrons

Electrons

Atomic Weight (AKA: Atomic Mass)

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11
Q

_____ 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

A

Isotopes, Same, Different

Same, Different

Radioisotopes

Half-Life

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12
Q

_____ ________ 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 ______

A

Mass Spectrometer

Same, Different

Protons, Neutrons

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13
Q

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

A

Laws of Conservation of Mass and Definite Proportions

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14
Q

Dalton’s Theory

1.) Each ______. is composed of tiny, indivisible particles called _____, which are ______ for that element but are ______ from atoms of other elements

A

Element

Atoms

Identical

Different

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15
Q

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 _____

A

Chemical, Atoms, Fixed, Molecule

Relative, Atoms

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16
Q

Dalton’s Theory

3.) No _____ are gained, lost, or changed in identity during a ______ reaction; they are just ______ to produce new substances

A

Atoms, Chemical, Rearranged

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17
Q

Law of Conservation of Mass

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

A

Detectable, Chemical

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18
Q

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 ______

A

Pure Compound

11.2%, 88.8%

Isotopes

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19
Q

Dmitri Mendeleev

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

A

Chemical, Physical

Predictable

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20
Q

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

A

Periods, Atomic Number

Groups

Chemical, Physical

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21
Q

Periodic Law

The ______ of elements are periodic functions of their ______ ______

(AN/AW example on PP slide 22)

A

Properties, Atomic Number

22
Q

Metals, Nonmetals, and Metalloids

Review Table on PP slides 23-24

A

Review Table on PP slide 23-24

23
Q

Solids, Liquids, and Gases

Review Table on PP slide 25

A

Review Table on PP slide 25

24
Q

Representative, Transition, and Inner Transition Elements

Review Table on PP slide 26

A

Review Table on PP slide 26

25
Q

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)

A

Chemical, Mixtures

Separated

Heterogenous or Homogenous

Compounds, Chemical

Homogenous

26
Q

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

A

(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)

27
Q

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

A

(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

28
Q

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

A

(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

29
Q

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

A

Molecule, Discrete

Molecular Formula, Atom

Nonmetals, Close

30
Q

Some Common Elements

Review PP slides 35-38

A

.

31
Q

Iron

Fe++ (Ferrous) and Fe+++ (Ferric) forms

Iron is vital for the transport of ____ in Hgb

Which form of Iron is preferred and why?

A

O2 (Oxygen)

Fe++ (Ferrous) is the preferred form of Iron because it has a better O2 carrying capacity in comparison to Fe+++ (Ferric)

32
Q

Methemoglobinemia

Causes and Treatment?

A

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

33
Q

Methemoglobinemia

Causes and Treatment?

A

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)

34
Q

What is the enzyme in the mitochondria that produces ATP?

A

Cytochrome Oxidase

35
Q

Molecular Elements

(Think number at bottom right)

Diatomic:

Tetratomic:

Octatomic:

See also: ____ and _____

A

H2, N2, O2, F2, Cl2, Br2

P4

S8

Nitrous Oxide (N20) and Nitric Oxide (NO)

36
Q

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”

A

Ionic, Oppositely

Crystalline Lattices

Cations, Anions, Discrete

37
Q

Chemically Inert Elements

Inert elements have their outermost energy level ( ____ ____) fully occupied by electrons

Number of electrons to complete valence shell is __

A

Valence Electrons

8

38
Q

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

A

Electrons

Electron Shells

Shell, Electrons

39
Q

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

A

Bonds, Electrons

Valence, Active

Octet, 2, 8

40
Q

Chemically Reactive Elements

Reactive elements have their outermost energy level fully occupied by __ electrons

A

8

41
Q

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

A

Transfer

Charged

Anion, Negative

Cation, Positive

42
Q

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)

A

Crystals

Crystals, Ionic

NaCl

43
Q

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 ______

A

Shared

Double or Triple

Molecules

44
Q

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

A

Equally, Nonpolar

Unequal, Polar

Polar, Dipole, Opposing

Water

45
Q

Covalent Bonds

____ distribution of charges

Hydrogen atoms form ____ bonds

Oxygen atoms form ____ bonds

Nitrogen atoms form ____ bonds

Carbon atoms form ____ bonds

A

Equal

Single

Two

Three

Four

46
Q

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)

A

Weak, Polar

Water

Surface Tension

Three-Dimensional

Collapse

47
Q

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)

A

Charge

Positive, Loss, Metals

Negative, Gain, Nonmetals

Representative

48
Q

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

A

Group, 8

“Ide”

Chloride ion, Sulfide ion, Nitride ion, Oxide ion

49
Q

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

A

Lower, Higher

Chromous ion versus Chromic ion

Ferrous ion versus Ferric ion

50
Q

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?

A

Discrete, Covalent

Water, Ammonia, Methane, Ethane, Propane, Nitrous Oxide

51
Q

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

A

Fixed, Water

Solid

Waters

52
Q

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 _______

A

Anhydrous, Hydrate, Scavenge

Silica

Reversible, Moisturizers

Chemistry/Physics Test 1 (2 decks)

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