Chapter 2 Atoms, Ions, Molecules

Question 0

What are the forms of matter?

Answer 0

• • Solid ( bone)
• • Liquid (blood)
• • Gas ( Oxygen/ Carbon Dioxide)

Question 1

Matter

Answer 1

Has mass, composed of atoms

Question 2

Atom ( smallest particle, make up everyday objects)

Answer 2

Building blocks of matter

Question 3

Name the subatomic particles?

Answer 3

• protons (+)
• neutrons (no charge)
• electrons (-)

Question 4

Atomic mass unit (AMU)

Answer 4

Mass of an atom

Question 5

Isotope

Answer 5

2 or more atoms of the same element have same # of protons but diff. # of neurons

Question 6

Radioisotope

Answer 6

Unstable, excess # of neurons

Question 7

Electron shell

Valence shell

Answer 7

• surround nucleus of shell

- outermost energy level

Question 8

Octet rule

Answer 8

Elements gain or lose electrons to keep their outer shell ( valence electron) full

Question 9

What is an inert element?

Answer 9

When the valence energy shell (outer shell) is full, they do not want to give, receive or share their electrons

Question 10

Ions 
Ionic Bond (Opposites attract)

Compound

Covalent bond

Answer 10

Atoms with charge
Attraction between 2 oppositely charged ions

Composed of 2 or more elements

Sharing of electrons

Question 11

Cation

Anions

Answer 11

Positive charge, Lose an electron

Negative charge, Gain an electron

Question 12

Molecule (a lot of ????)

Molecular compound (combined)

Answer 12

2 or more atoms joined by a chemical bond

Composed of two or more different elements

Question 13

Molecular formula

Structural formula (made of)

Isomers (same but different)

Answer 13

Chemical constituents of a molecule

Shows # & types of atoms, also their arrangement in a molecule

Molecules with same #, & kind of elements, arranged differently

Question 14

Single Covalent Bond

Double Covalent Bond

Triple Covalent

Answer 14

One pair of electron shared between 2 atoms

Sharing of 2 pairs of electrons between 2 atoms

3 pairs of electrons shared between atoms

Question 15

Nonpolar covalent bond (equal)

Polar covalent bond (unequal)

Amphipathic Molecules (both)

Answer 15

Share electrons equally (charged atom)

Unequal sharing of electrons by atoms (positive atom, negative atom)

Molecules that Contain polar & non polar components

Question 16

Intermolecular attractions

Hydrogen bond (polar molecules)

Electronegativity

Answer 16

Weak chemical attractions to other molecules

Weak attraction between partially (+) &partially (-) hydrogen atom in a molecule

Ability to attract

Question 17

What are properties of water? (5)

Answer 17

1) high heat capacity- takes a lot of heat to raise temp.
2) high heat vaporization- a lot of heat is needed to break something down
3) polar solvent properties/ universal solvent- many things can be dissolved in water
4) reactivity- necessary part of hydrolysis & dehydration synthesis
5) cushioning- resilient cushion around certain body organs

Question 18

Electrolytes

(Ex: salts, acids, bases

Answer 18

Dissolve & dissociate in water

Question 19

Neutralization Reaction

Answer 19

solution is acidic or basic and returned to neutral (ph7)

Question 20

Buffer, describe the action.

Example or weak acid/ base

Answer 20

• single or group of substances that help prevent ph changes
• Release hydrogen ions if Ph rises, bind or accept hydrogen ions if ph falls

-Carbonic (weak acid)
-Bicarbonate (weak base)
Present in blood & serve as buffers to keep pH normal

Question 21

Mixture

Answer 21

2 or more components physically mixed ( not chemically bonded)
Ex, sugar & water

Question 22

Examples of mixtures:

Answer 22

1) suspensions- heterogenous mixed, worst mixed, so lutes will separate
2) colloids-heterogeneous mixture, solutes will not settle out, appears milky
3) solutions- homogeneous mixture, best mixed, can’t see different parts

Question 23

Emulsion (forced)

Answer 23

Combo of water & non polar (fats) liquid forcibly mixed

Question 24

Explain different ways to express concentration of solute in a solution

Answer 24

Mass/ volume- mass of solute per volume of solution(blood test r measured)
Mass/volume percent- grams of solute per 100 mL of solution (IV solution)
Molarity- # of moles per liter of solution
Molality- moles per kg of solvent

Question 25

Monomer (one)

Polymer (many)

Examples of function al groups (6)

Answer 25

Molecule that may chemically bind to other molecules

Large molecules or macromolecules composed of repeated subunits

Hydroxyl, Carbonyl, Carboxyl, Amine, Phosphate, Sulfhydryl

Question 26

Dehydration Synthesis (remove water, to make)

Hydrolysis (add water, break up)

Answer 26

• 2 molecules are joined to make a larger one

- larger molecules are broken down

Question 27

Organic macromolecules

Answer 27

• lipids (fats)
• carbohydrates ( starches, corn)
• nucleic acid ( DNA & RNA)
• Proteins (muscle tissue)

Question 28

4 types of lipids and roles

Answer 28

• triglycerides or neutral fats- long term energy storage
• Phospholipids- control movement through membranes
• Steriods- cholesterol, steroid cholesterol & bile salts HDL, bad/. LDL, good
• Eicosainodes- Rollin in blood clotting, control BP, inflammation, labor contractions

Question 29

Carbohydrates (sugars, starches)

3 classes of carbohydrates

Answer 29

– monosaccharides (glucose, fructose, galactose)
Gives quick energy
– disaccharides ( sucrose, lactose, maltose)form from 2 monosaccharides
– polysaccharides ( starch, glycogen, cellulose) formed from MANY monosaccharides

Question 30

Nucleic acids ( DNA & RNA)

What. Akers up a nucleotide?

Answer 30

Store & transfer genetic or hereditary information within cells

• sugar, phosphate, nitrogenous base ( gas)

Question 31

Acids (H+)

Base

Answer 31

Dissociates in water to produce H+ & anion

Accepts H+ when added to a solution