Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > Chemistry Review Week 5 > Flashcards

Chemistry Review Week 5 Flashcards

You may prefer our related Brainscape-certified flashcards:
Chemistry 101 flashcards Periodic Table flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

What is chemistry?

A

The study of matter and it’s changes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is matter?

A

Anything that has mass and occupies space

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What are atoms

A

Building block of matter

Comprised of protons neutrons and electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What are neurons

A

They have a neutral charge

Mass = 1 amu

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What are electrons

A

They have a negative charge

  • mass is irrelevant
  • Number of electrons will match the number of protons
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What are ions

A
  • atoms/groups of atoms bonded together with a net charge
  • cations: positive
  • anions: negative
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What are elements

A

Only one type of atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What are compounds

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What are molecules

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Can a substance be both a molecule and an element

A

Yes

Oxygen is an example

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is a physical change

A

No change in chemical make up

Example: Melting ice

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is a chemical change

A

Always makes a chemically different substance

Example: 2H2O——->2H2 = O2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is a chemical property

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What determines an atoms identity?

A

Atomic number (Z)

  • the number of protons determines identify

Ex: carbon Z = 6

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

How is atomic mass measured?

A
  • atomic mass unit (amu)

- protons and neutrons - 1amu

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What are isotopes?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions