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Intro to Biology for Vet Techs > Chemistry > Flashcards

Chemistry Flashcards

1
Q

the study of matter, its chemical and physical properties and the chemical and physical changes it undergoes

A

Chemistry

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2
Q

a specific substance that can’t be broken down into simpler substances by chemical reactions

A

Element

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3
Q

How many elements are on the periodic table? How many are naturally occurring? How many are unstable?

A

118 total
94 naturally occurring
24 unstable

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4
Q

the arrangement of the elements that communicates important information about each of the elements and how they relate to one another

A

Periodic Table

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5
Q

What 4 things are included in each square on the periodic table?

A
  1. Atomic Number
  2. Chemical Symbol
  3. Element Name
  4. Atomic Mass
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6
Q

What does the Atomic Number represent?

A

protons in an atom of an element

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7
Q

How is the Atomic Mass calculated?

A

Atomic Mass = # proton + average # neutrons

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8
Q

How do you calculate the average number of neutrons?

A

Average # Neutrons = Rounded Atomic Mass - Atomic Number

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9
Q

the smallest component of an element that retains all of the chemical properties of that element

A

Atom

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10
Q

the central region of all atoms that contain protons + neutrons and are orbited by electrons on the outside

A

Nucleus

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11
Q

positively charged particles inside the nucleus of an atom

A

Protons

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12
Q

negatively charged particles that orbit around the outside of the nucleus of an atom

A

Electrons

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13
Q

particles with no charge inside the nucleus of an atom

A

Neutrons

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14
Q

electrons in the outer electron shell and are important for chemical reactions

A

Valence Electrons

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15
Q

Balanced atoms have what electron to proton ratio?

A

1:1
Atoms have the same # of electrons as protons

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16
Q

atoms of the same element that have the same number of protons but a different number of neutrons

A

Isotopes

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17
Q

How do you write proton vs electron charges?

A

Proton = +1
Electron = -1

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18
Q

when an atom contains an equal number of protons and electrons

A

Neutral Atom

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19
Q

Isotopes of an element are chemically _____ , BUT may have ______ stabilities

A

identical
different

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20
Q

How would you write normal magnesium (atomic mass of 24) vs an isotope of magnesium (atomic mass of 25)? And how many protons and neutrons would each have?

A

Mg-24
12 protons + 12 neutrons

Mg-25
12 protons + 13 neutrons

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21
Q

holds the atoms of two joined elements together

A

Chemical Bond

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22
Q

What part of the atom forms bonds?

A

Electrons

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23
Q

How many electrons can the first 3 orbitals hold?

A

First - 2
Second - 8
Third - 18

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24
Q

What is it called when the outer orbital is full?

A

Octet

25
Q

How can atoms become more stable?

A

By filling their outermost orbital through the loss, gain or sharing of valence electrons via chemical bonds

26
Q

What are the 3 main kinds of bonds?

A
  1. Ionic Bonds
  2. Covalent Bonds
  3. Hydrogen Bonds
27
Q

type of bond that involves one atom losing 1 or more electrons and another atom gaining the electrons that were lost by the first atom

A

Ionic Bond

28
Q

What does an atom become once it has a charge?

A

Ion

29
Q

What are the 2 types of ions and what is the difference?

A
  1. Anions = ions with a negative charge
  2. Cations = ions with a positive charge
30
Q

the result when 2 ions attract to each other and stick together to make a bond

A

Ionic Compound

31
Q

Ionic Compounds must contain how many different elements?

A

At least 2

32
Q

when elements share electrons to achieve a full outer shell instead of gaining or losing electrons

A

Covalent Bonds

33
Q

How many bonds can there be in Covalent Bonds and how many electrons are involved?

A

Three: single, double, and triple Covalent bonds

Single Covalent Bonds - 1 electron
Double Covalent Bonds - 2 electrons
Triple Covalent Bonds - 3 electrons

34
Q

the result when atoms are joined by covalent bonds

A

Molecule

35
Q

How many different elements must Molecules contain?

A

Don’t have to contain different elements - can be multiple atoms of the same element

36
Q

All _____ are _____, but not all ______ are _____.

(molecules/compounds)

A

All compounds are molecules BUT not all molecules are compounds

37
Q

What are the 2 types of Covalent Bonds?

A
  1. Nonpolar
  2. Polar
38
Q

when 2 bonded atoms share electrons nearly [equally]

A

Nonpolar Covalent Bond

39
Q

when 2 bonded atoms share the electrons [unequally] due to a difference in charge between them

A

Polar Covalent Bond

40
Q

Give an example of a Nonpolar Covalent Bond vs a Polar Covalent Bond?

A

Nonpolar - O2 (the 2 oxygen atoms are identical and thus the electrons are shared equally)

Polar - H2O (the electrons are pulled closer to the oxygen atom, thus the oxygen end of the molecule is slightly negative and the hydrogen end is slightly positive)

41
Q

created when a molecule has regions of charge that are separated

A

Dipole

41
Q

molecules with dipoles

A

Polar Molecules

42
Q

a weak attraction between an electronegative atom in one molecule and an electropositive ____ atom already bonded to an electronegative atom in another molecule

A

Hydrogen Bond

43
Q

How are hydrogen bonds indicated on models?

A

Dashed line

44
Q

What is the universal solvent and why is it called that?

A

Water - capable of dissolving more chemicals than any other solvent

45
Q

What types of molecules can water dissolve?

A

Polar only

Nonpolar molecules like fats and oils cannot be dissolved in water

46
Q

how well molecules are attracted to themselves

A

Cohesion

47
Q

how well molecules are attracted to other substances

A

Adhesion

48
Q

What are 4 important properties of water that are caused by hydrogen bonding and the polarity of water?

A
  1. Universal Solvent
  2. Cohesion
  3. Adhesion
  4. High boiling and melting points
49
Q

a substance that releases hydrogen ions (H+) and thus increases the concentration of (H+) in the solution

A

Acid

50
Q

have an excess of hydrogen ions or hydronium ions and have a LOW pH value

A

Strong Acids

51
Q

a substance that releases hydroxide ions (OH-) or other (-) charged ions that combine with hydrogen ions, reducing their concentration in the solution

A

Base

52
Q

have an excess of hydroxide ions and have a HIGH pH value

A

Strong Base

53
Q

a solution that is not acidic or basic

A

Neutral

54
Q

a measurement scale that indicates a solution’s acidity or alkalinity on a scale from 0 to 14

A

pH

55
Q

What is the pH formula and it can be rearranged to solve for what?

A

pH = -log[H+]

The Hydrogen Ion Concentration

56
Q

Chemistry terms for how acidic or basic a solution is

A

Acidic = Acidity
Basic = Alkalinity

57
Q

What is the pH inside human cells and blood?

A

Close to neutral

58
Q

the process by which neutral atoms/molecules are converted to electrically charged atom/molecules through gaining or losing electrons

A

Ionization

Intro to Biology for Vet Techs (12 decks)

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