Lecture Series 2 Basic Chemistry Vocabulary Flashcards

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1
Q

atom

A

The smallest unit of an element that retains the element’s distinctive properties. Atoms are the building blocks of all matter.

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2
Q

proton

A

A subatomic particle, it is the positively charged particle found in the nucleus of an atom.

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3
Q

neutron

A

A subatomic particle, it is an electrically neutral particle found in the nucleus of an atom.

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4
Q

electron

A

A subatomic particle, it is a negatively charged particle found outside the nucleus of an atom.

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5
Q

atomic number

A

The number of protons in an atom’s nucleus.

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6
Q

molecule

A

an association of atoms held together by nuclear bonds

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7
Q

element

A

a pure substance that has distinctive physical and chemical properties, and cannot be broken down into other substances by ordinary chemical methods.

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8
Q

ion

A

an atom that has lost or gained electrons and therefore is either negatively or positively charged

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9
Q

isotope

A

two or more forms of an element that have the same number of protons but different numbers of neutrons

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10
Q

chemical reaction

A

the process of breaking existing chemical bonds and creating new ones

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11
Q

chemical bond

A

a force that holds two atoms together

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12
Q

ionic bond

A

the chemical attraction between a negatively charged ion and a positively charged ion

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13
Q

covalent bond

A

the sharing of electrons between two atoms

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14
Q

polar molecule or dipole

A

a molecule whose electrical charge is shared unevenly, with some regions being electrically negative and others being electrically positive

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15
Q

hydrogen bonding

A

the weak electrical attraction between a hydrogen atom with a partial positive charge and a neighboring atom with a partial negative charge

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16
Q

pH scale

A

a logarithmic scale that indicates the concentration of hydrogen ions. The scale goes from 0-14 with 0 representing an extremely high concentration of free H ions and 14 representing the lowest concentration.

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17
Q

hydrophobic

A

literally “water fearing.” Excluded from water

18
Q

hydrophilic

A

literally “water loving.” Soluble in water.

19
Q

atomic nucleus

A

the small, dense region consisting of protons and neutrons at the center of an atom

20
Q

compound

A

a mixture that is composed of two or more separate elements and contains more than one type of atom bonded together, ex. phytochemicals and buffers

21
Q

electron shell

A

the outside part of an atom around the atomic nucleus. It is a group of atomic orbitals with the same value of the principal quantum number n. Electron shells have one or more electron subshells, or sublevels

22
Q

electron fill order

A

First electron shell can hold up to 2 e-•2nd electron shell can hold up to 8e-•3rd electron shell can hold up to 18e-•4th electron shell can hold up to 32e-•However, 3rd and 4th shells will not fill with more than 8 electrons until all 18 or 32.

23
Q

electron frequency

A

the energy of an electron expressed as light

24
Q

free radicals

A

a molecule used within the biochemical pathways of cells that has lost an electron and therefore will steal an electron from the closest molecule; can set off a chain reaction – resulting in cell death and even tissue damage

25
Q

metallic bond

A

Electron pooling, the force of attraction between valence electrons and the metal atoms. It is the sharing of many detached electrons between many positive ions, where the electrons act as a “glue” giving the substance a definite structure. It is unlike covalent or ionic bonding

26
Q

polar covalent bond

A

a particular type of covalent bond. In a polar covalent bond, the electrons shared by the atoms spend a greater amount of time, on the average, closer to the Oxygen nucleus than the Hydrogen nucleus; When two atoms are bonded and their nucleus contains different numbers of protons

27
Q

nonpolar covalent bond

A

a type of chemical bond where two atoms share a pair of electrons with each other. Polar covalent bonding is a type of chemical bond where a pair of electrons is unequally shared between two atoms.

28
Q

polar molecule (dipole)

A

a net dipole as a result of the opposing charges (i.e. having partial positive and partial negative charges) from polar bonds arranged asymmetrically. Water (H2O) is an example of a polar molecule since it has a slight positive charge on one side and a slight negative charge on the other.

29
Q

nonpolar molecule

A

A molecule may be nonpolar either when there is an equal sharing of electrons between the two atoms of a diatomic molecule or because of the symmetrical arrangement of polar bonds in a more complex molecule.

30
Q

cohesion

A

Ability of water molecules to cling to each other due to hydrogen bonding

31
Q

adhesion

A

Ability of water molecules to cling to other polar surfaces

32
Q

pH

A

Mathematical way to indicate the number of hydrogen ions in solution; pH (potential of hydrogen) is a scale of acidity from 0 to 14. It tells how acidic or alkaline a substance is. More acidic solutions, have lower pH

33
Q

buffer

A

a compound that accepts H+ in response to a pH change. Theses chemicals or combination of chemicals keeps pH within normal limits; Resists pH change by taking up excess H+ or OH-; pH of blood is about 7.4 – maintained by buffers – the main one is the bicarbonate ion.

34
Q

dissociation

A

the disconnection or separation of something from something else; Water, which not only dissolves many compounds but also dissolves more substances than any other liquid, is considered the universal solvent. A polar molecule with partially-positive and negative charges, it readily dissolves ions and polar molecules; Due to polarity and H-bonding, water dissolves many substances

35
Q

hydration

A

a term used to indicate that a substance contains water; When table salt (NaCl) is mixed in water, spheres of hydration form around the ions. Since many biomolecules are either polar or charged, water readily dissolves these hydrophilic compounds.

36
Q

surface tension

A

the elastic tendency of a fluid surface which makes it acquire the least surface area possible. … At liquid–air interfaces, surface tension results from the greater attraction of liquid molecules to each other (due to cohesion) than to the molecules in the air (due to adhesion). Water has a high surface tension - Water molecules at the surface cling more tightly to each other than to the air above mainly due to hydrogen bonding

37
Q

specific heat of water

A

The specific heat of water is called the calorie (not the same as kilo calories in food), and it is the amount of heat energy needed to raise 1 gram of a substance by 1 degree celsius. Water has a higher specific heat than sand, for example. It takes more heat energy to raise the temperature of water than it does to raise the temperature of sand.

38
Q

heat capacity

A

The capability of a substance to absorb heat energy; The many hydrogen bonds linking water molecules allow water to absorb heat without greatly changing its temperature.

39
Q

heat of vaporization

A

the amount of energy (enthalpy) that must be added to a liquid substance, to transform a quantity of that substance into a gas; Takes a great deal of energy to break H bonds for evaporation, heat is dispelled as water evaporates

40
Q

heat of fusion

A

opposite of heat of vaporization and is the amount of heat energy must withdraw to cause water to freeze or change from liquid to solid.

41
Q

density

A

the degree of compactness of a substance

42
Q

subatomic particle

A

the three components of an atom, the proton, neutron, and electron