Chapter 2

Question 1

What is a compound?

Answer 1

2 or more kinds of atoms

Question 2

What is a proton?

Answer 2

positive charge

Question 3

What is a neutron?

Answer 3

neutral charge

Question 4

What is an electron?

Answer 4

negative charge

Question 5

Physical change

Answer 5

• No change in substance identity (e.g. melting ice)

Question 6

What is matter?

Answer 6

anything that has mass and occupies space

Question 7

Physical Chemistry

Answer 7

Theoretical models to explain chemical systems

Question 8

What is chemistry?

Answer 8

study of matter and changes it undergoes

Question 9

Why is mass spectroscopy important in anesthesia?

Answer 9

• It is part of the anesthesia machine.
• Offers real time monitoring
• identify something we didn’ expect are benefits

Question 10

What is hexa and hepta?

Answer 10

6, 7

Question 11

Ionization Energy

Answer 11

measure tendency of neutral atom to resist loss of electrons

Question 12

positively charged ions formed when an atom or molecule loses electrons

Answer 12

cation

Question 13

negatively charged ions that gains electrons

Answer 13

anion

Question 14

Inorganic Chemistry

Answer 14

Study of non carbon based elements

Question 15

Organic Chemistry

Answer 15

Study of carbon based compounds

Question 16

Biochemistry

Answer 16

Chemistry within living things. Important in physiology and pharmacology

Question 17

Chemical change

Answer 17

chemical change always result in formation of chemically different substances (rusting iron)

Question 18

Intensive (physical property)

Answer 18

Independent of amount (e.g. density)

Question 19

Extensive (physical property)

Answer 19

dependent on amount (e.g. mass)

Question 20

Chemical Property

Answer 20

describe how a substance reacts chemically (e.g flammability)

Question 21

Physical Property

Answer 21

Observable without changing chemical identity (color, melting point)

Question 22

+1 charge, 1 amu

Answer 22

Proton

Question 23

0 charge, 1 amu

Answer 23

Neutron

Question 24

-1 charge, negligible mass

Answer 24

electrons

Question 25

Dense core containing protons and neutrons

Answer 25

Nucleus

Question 26

(...) occupy orbitals, governed by quantum mechanics

Answer 26

Electrons

Question 27

An (...) contains substance made of one type of atom

Answer 27

Element

Question 28

A (...) is a substance with two or more types of atoms bonded

Answer 28

compound

Question 29

A (...) is a electrically neutral group of atoms bonded by covalent bonds

Answer 29

Molecule

Question 30

(...) are made of ions; not molecular; form crystalline lattices

Answer 30

Ionic compounds

Question 31

(...) cannot be physically separated (e.g. water, NaCl)

Answer 31

Pure Substances

Question 32

(...) are physically combined substances

Answer 32

Mixture

Question 33

(...) have uniform composition (e.g. saline)

Answer 33

homogenous mixture

Question 34

(...) has visible phase boundaries (e.g. blood)

Answer 34

Heterogenous mixture

Question 35

Atomic Number (Z) =?

Answer 35

of Protons

Question 36

Mass # (A) =?

Answer 36

Protons + Neutrons

Question 37

Same atomic number (Z), but different mass number (A). Example: C-12 and C-14

Answer 37

Isotopes

Question 38

Dalton's Atomic Theory

Answer 38

-All matter is made of atoms - Atoms of the same element are identical - compounds form in fixed ratios - Atoms are rearranged, not created nor destroyed, in chemical reactions - Modern updates: subatomic particles and isotopes were later discovered

Question 39

Ionization energy trends on periodic table

Answer 39

Increases from left to right and bottom to the top

Question 40

- Made of nonmetals - Use prefixes mono, di, tri, tetra, penta - Add suffix "ide" (e.g. CO2, carbon dioxide)

Answer 40

Molecular Compounds

Question 41

- Made of metal and non-metal - Name: cation + anion (e.g. NaCl, sodium chloride) - Transition metals: use roman numerals for charge (e.g. FeCl3, Iron(III) chloride)

Answer 41

Ionic Compounds

Question 42

-charged groups of atoms (e.g SO4^2- = sulfate, NO3^- = nitrate) - "-ate" = more oxygen, "-ite" = fewer oxygen atoms

Answer 42

Polyatomic ions

Question 43

- Ionic compounds with water (e.g. CuSO4*5H2O = copper(II) sulfate pentahydrate) - "Anhydrous" = water removed, "Hygroscopic" = absorbs water from air

Answer 43

Hydrates

Question 44

Electrolytes vs. Nonelectrolytes

Answer 44

- Electrolytes conduct electricity in solution (e.g. NaCl) - Non electrolytes do not conduct electricity (e.g. sugar)

Question 45

Importance of electrolytes in anesthesia?

Answer 45

- IV fluids and medications often contain electrolytes - Understanding their behavior is crucial for fluid/electrolyte balance

Question 46

Mole = mol: 6.022x10^23 particles

Answer 46

Avogrado's Number

Question 47

- g/mol = atomic/molecular weight - used to convert between grams and moles

Answer 47

Molar Mass

Question 48

- Quantitative relationships in chemical reactions - Basic steps: balance chemical equation, convert grams to moles using molar mass, use mole ratios to solve for unknowns, convert back to grams if needed - Clinically relevant

Answer 48

Stoichiometry

Question 49

According to Dalton's Atomic Theory, what happens to atoms in chemical reactions?

Answer 49

Atoms are rearranged, not created or destroyed.

Question 50

What is the Law of Conservation of Mass?

Answer 50

No detectable change in mass; components are neither created nor destroyed in a chemical reaction.

Question 51

How are Ionic Compounds typically named?

Answer 51

Cation name + Anion name (e.g., Sodium Chloride).

Question 52

When naming ionic compounds with Transition Metals, what is used to indicate the charge?

Answer 52

Roman numerals (e.g., Iron (III) Chloride).

Question 53

What does 'Hygroscopic' mean regarding hydrates?

Answer 53

Absorbs water from the air.