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Chemistry > Chemistry Review Week 5 > Flashcards

Chemistry Review Week 5 Flashcards

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1
Q

What is chemistry?

A

The study of matter and it’s changes

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2
Q

What is matter?

A

Anything that has mass and occupies space

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3
Q

What are atoms

A

Building block of matter

Comprised of protons neutrons and electrons

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4
Q

What are protons

A

They have a positive charge
The atomic number (Z) number of protons, determines identity of the atom
-mass = 1 atomic mass unit (amu)
-number of proton will match the number of electrons

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5
Q

What are neurons

A

They have a neutral charge

Mass = 1 amu

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6
Q

What are electrons

A

They have a negative charge

  • mass is irrelevant
  • Number of electrons will match the number of protons
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7
Q

What are ions

A
  • atoms/groups of atoms bonded together with a net charge
  • cations: positive
  • anions: negative
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8
Q

What are elements

A

Only one type of atom

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9
Q

What are compounds

A

More than one kind of atom in a fixed ratio by mass

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10
Q

What are molecules

A

Groups of atoms chemically bonded together in a discrete unit by covalent bonds
-neutral charge

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11
Q

What are ionic compounds

A

Contain both positive and negatively charged ions with no identifiable units
-attached by charge and are not molecules

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12
Q

Can a substance be both a molecule and an element

A

Yes

Oxygen is an example

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13
Q

What is a physical change

A

No change in chemical make up

Example: Melting ice

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14
Q

What is a chemical change

A

Always makes a chemically different substance

Example: 2H2O——->2H2 = O2

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15
Q

What is a physical property

A

Maybe observed or measured without changing the chemical make up

  • intensive: integral to the material, regardless of amount (ex: color)
  • extensive: depends on sample size (ex: volume)
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16
Q

What is a chemical property

A

Describes the type of chemical changes the material tends to undergo
Ex: flammable

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17
Q

What are substances

A

Pure materials that can’t be physically separated into similar components

  • throughout all samples the chemical and physical properties are uniform
  • compound or element
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18
Q

What are mixtures

A

Two or more pure substances

  • physical processes can separate the mixture into simpler substances
  • homogenous: uniform in physical and chemical properties throughout the whole sample (ex: normal saline)
  • heterogeneous: distinct phases boundaries where chemical and/or physical properties change (ex: emesis)
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19
Q

Describe the atomic structure

A
  • protons and neutrons on the nucleus
  • electrons surround the nucleus in cloud-like orbitals
  • have wave-like properties rather than geometric properties
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20
Q

What determines an atoms identity?

A

Atomic number (Z)

  • the number of protons determines identify

Ex: carbon Z = 6

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21
Q

What is mass number (A)?

A 
Mass number (A) = Z + N
-mass number can never be smaller than the atomic number

Z: atomic number
N: neutron number

-the mass number can never be smaller than the atomic number

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22
Q

How is atomic mass measured?

A
  • atomic mass unit (amu)

- protons and neutrons - 1amu

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23
Q

What are isotopes?

A

Same atomic number, different mass number (different number of neutrons, same protons)

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24
Q

What is Dalton’s Atomic Theory?

A
  1. Elements are composed of tiny, indivisible particles called atoms, all atoms of a given element are identical and unique to the element
  2. Compounds are formed by bonding atoms together in a fixed ratio
  3. Chemical reactions do not create, destroy, or change atoms into atoms of other elements. Chemical reactions cause atoms to recombine into new substances
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25
Q

What is the Law of Conservation of Mass?

A
  • No detectable change in total mass occurs during a chemical reaction
  • the components are neither created, nor destroyed. They recombine.
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26
Q

What is the Law of Definite Proportions?

A

-different samples of a pure compound always contain the same elements in the same proportion by mass

Ex: water = 11.2% hydrogen and 88.8% oxygen by mass

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27
Q

What is the law of multiple proportions

A

-some elements can combine to give more than one compound.

Ex: carbon burned in O2 produces both CO2 and CO

28
Q

What are the flaws in Dalton’s theories?

A
  • not all atoms of an element are identical isotopes
  • atoms are comprised of even smaller particles and nuclear processes convert atoms of one element into atoms of another element
29
Q

What is periodic law?

A

Properties of elements are periodic functions of their atomic numbers

30
Q

Describe the periodic table

A

-chemical and physical properties repeat in a regular pattern
-in order of increasing atomic number
-vertical: groups/families
-similar chemical and physical properties
-rows: periods
-adding electrons to energy levels, electron shells
-the element at the end of the row has the outer shell full of electrons
Which means that they are stable

31
Q

What determines if an element accepts or releases electrons?

A
  • elements with a nearly full electrons shell accept electrons, anions
  • elements with nearly empty electron shells readily release elections, cations
32
Q

What are atomic weights?

A

-the weight of the periodic table is average of all isotopes

33
Q

What are the periodic table classifications?

A
  • representative elements: In the high rises on the left and right
  • transition elements: Connector between the representative elements
  • inner transition elements: those at the bottom of the table
  • most elements are metals and are on the left side of the table.
  • non-metals are on the right side of the table
  • metalloids: along the ladder
34
Q

What are characteristics of metals?

A
  • shiny luster
  • ductile (can draw out into thin wire)
  • malleable
  • good conductors of heat and electricity
  • react to form cations by giving away electrons
35
Q

What are characteristics of non-metals?

A
  • liquids, solids, or gases
  • solids tend to be brittle
  • do not conduct
  • tend to form anions
36
Q

What are characteristics of metalloids?

A
  • intermediates
  • shiny luster
  • less malleable and ductile than metals
  • conduct electricity but not well —>semiconductors

-silicone is an example

37
Q

What state are more elements in on the periodic stable?

A

Most are solids

38
Q

What are the 2 liquids on the periodic table?

A

Mercury and bromium

39
Q

What element will melt in your hand?

A

Gallium

40
Q

What elements are gases?

A

Hydrogen, nitrogen, oxygen, fluorine, chlorine and all Noble Gases are gases

41
Q

What are electrolytes?

A

A substance that dissolves in water to give a solution conductivity.

  • most molecular compounds are non-electrolytes
  • dissolution happens by water interacts very effectively with ions
  • water itself is non-electrolytes
42
Q

Aluminum (Al)

A
  • found it antiperspirants and antacids
  • does not occur naturally, must be synthesized
  • avoid in dialysis pts bc it will build up in their system and cause neurological problems
43
Q

Barium (Ba)

A
  • used in radio graphic GI studies will use barium sulfate oral solution or enemas
  • toxic, but pts will excrete the material fairly easily
  • does not absorb in GI tract
44
Q

Calcium (Ca)

A
  • found in antacids, phosphate binders
  • doesn’t occur naturally in nature in the elemental form
  • essential for muscle contraction, bone stability
  • will cause constipation
  • bill bind to phosphorous
  • if albumin is low, Ca will look falsely low
45
Q

Carbon (C)

A
  • activated charcoal: used in overdoses
  • in most compounds, highly versatile
  • graphite and diamond occur naturally
  • has 4 binding sites
46
Q

Chlorine (Cl)

A
  • Clorox, other cleaners
  • disinfectant
  • toxic green gas
47
Q

Chromium (Cr)

A

-found in stainless steel

48
Q

Copper (Cu)?

A
  • great conductor

- reddish metal

49
Q

Fluorine (F)

A
  • neurotoxin. Believe it may be adding to autism and ADD/ADHD
  • sodium fluoride strengthens teeth
50
Q

Helium (He)

A
  • colorless, inert gas

- MRI coolant

51
Q

Hydrogen (H)

A

-most common atom in the universe
(>95% of all known matter)
-colorless, flammable gas
-it easy to add onto stable an element

52
Q

Iodine (I)

A
  • found in topical antiseptics and anti thyroid medications

- purplish/black solid

53
Q

Iron (Fe)

A
  • found in each hemoglobin molecule to transport oxygen through the blood
  • metal

PPIs reduce the absorption of iron, calcium, and other minerals

54
Q

Lithium (Li)

A
  • used as a mood stabilizer for bipolar pts

- silvery, highly reactive metal

55
Q

Magnesium (Mg)

A
  • important for cardiac conduction and potassium levels
    • must correct Mg level before you replace k)
  • laxative
  • tocolytic therapy: means used to help delay pre-term delivery
  • silvery white metal
56
Q

Nitrogen (Ni)

A
  • 80% of air
  • found in anesthetic gas as nitrous oxide (N2O)
  • odorless, colorless gas
57
Q

Oxygen (O)

A
  • strong tendency to accept electrons
  • important in ATP synthesis
  • odorless, colorless, reactive gas
58
Q

Phosphorus (P)

A
  • found in RNA and DNA and in ATP
  • low phos may cause brittle bone and respiratory failure
  • supplemented in salt forms with sodium or potassium

***refeeding syndrome: start feeding slow so that body doesn’t pull in excess minerals/electrolytes (potentially fatal shift of fluid and electrolytes)

59
Q

Potassium (K)

A
  • important for muscle contraction
  • effected by ACE inhibitors, loop diuretics
  • inverse relationship with insulin
  • silvery white metal, highly reactive
60
Q

Sodium (Na)

A
  • CNS stability, water balance
  • muscle contractions
  • can not change sodium levels rapidly bc water will shift too quickly and alter brain mass and cause permanent damage+ sz
  • sodium and water follow each other
61
Q

Titanium (Ti)

A
  • found in prosthetic implants
  • lightweight, low toxicity, high strength
  • grayish metal
62
Q

Zinc (Zn)

A
  • calamine lotion, sunblock, wound healing, cold symptom relief
  • bluish silver metal
63
Q

What are molecular compounds?

A

Only composed of nonmetals (right side of the periodic table)
-easier to name

64
Q

What are ionic compounds?

A

-almost always comprised of a metal and nonmetal

65
Q

What are ionic compounds sometimes referred to as?

A

Salts
-reactions of an acid with a base

Monatomic cations of representative metals

  • almost always form cations with the charge group = group number
  • group number = # of elections in the outermost shell
  • losing elections lead to a configuration identical to the closest Nobel gas
  • ionic charges >+3 are not observed and and impossible to maintain
  • group 1A = +1, Group 2A = +2, Aluminum = +3

Chemistry (7 decks)

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