Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

HESI-A2 > Chemistry > Flashcards

Chemistry Flashcards

(85 cards)

Start Studying
1
Q

Why does chemical bonding happen?

A

They form to make atoms more stable; atoms are “stable” when the outer orbital is “full”.

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

Ionic Bonds

A

One atom wants to give away an electron and one wants to take that electron so both are stable. Due to now opposite charges the two atoms stick together.
-Ex: Na ( has 1 electron, is neg. ) +Cl ( has 7 electrons, is pos. ) = Na ( becomes + cation, no ele. so is stable ) + Cl ( becomes - anion, has 8 ele. so is stable ).

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

Covalent Bonds

A

Atoms share electrons to become stable. Strongest bond that is not an IMF!

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

Polar Covalent Bonds

A

When the atoms are sharing electrons and the atoms have different charges.

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

Single Bonds

A

Only one pair of electrons is shared between two or more atoms ( only 2 electrons are shared ).
-Ex: H-O-H ; dashes represent single bonds.

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

Double bonds

A

Two pair of electrons are being shared ( 4 electrons involved ).
-Ex: O2 equals O=O ; two lines represents double bond.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Salts

A

Are formed from the remaining ions that do not form H2O ( acids + bases = try to neutralize each other and form H2O ).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Acids

A

Compounds that produces excess H+ ions.

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

Bases

A

Compounds that produce excess OH- ions.

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

Acid-Base concentration ( how is the acid-base measured )

A

Can be measured by the pH scale.

-Ex: 0-14; 0-6 is acidic, 7 is neutral, and 8-14 is basic.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Hydrochloric acid ( HCL )

A

Abundant amount of hydrogen chloride in water. Found in gastric juices; when not in gastric juices it is highly corrosive.

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

Liquid Drug Forms

A

Packaged in prefilled containers of stalk bottles.
Administered w/ : cups, teaspoons, needles attache to tubing or syringes, needle-less syringes, drops in mouth/eyes/ears, NG tubes.

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

Aqueous

A

Supplied in H2O-based solution,

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

Elixir

A

Sweetened w/ alcohol.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Emulsion

A

Mixture of 2 liquids that normally do not mix ( oil & water ).

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

Fluid

A

All liquid medications.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Drops

A

Liquid drops.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Half-strength

A

Solution has been diluted 50%.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Mixture

A

Compound medication consisting of more than one liquid medication.

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

Solution

A

H2O based liquid medication.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Suspension

A

Solid particles in a liquid medication that must be shaken gently & thoroughly

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

Atoms

A

Basic building blocks.
Nucleus contains ( + charges ) protons and neutrally charged neutrons.
Electrons ( - charged ) are on the outside of the nucleus.
Electrically neutral : atoms are - when more electrons than protons; atoms are + when more protons than electrons.

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

Atomic number

A

Number of protons in the nucleus. ( Above element symbol )

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Atomic Mass

A

Number of protons and neutrons combined; or average mass of atoms isotopes. ( Below element symbol ).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Orbitals
- Each orbital holds 2 electrons. Also arranged in energy levels. - Number = orbital #; letter= sublevel identification. - Sublevels: S= 1 orbital ( 2 electrons ), P= 3 orbitals ( 6 elec. ), D= 5 orbitals ( 10 elec. ), F= 7 orbitals ( 14 elec. ). - Arrangement: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 7s, 5f, 6d, 7p.
26
Energy levels
Energy level closet to the nucleus holds 1 orbital ( so only 2 electrons ). All other energy levels have 4 orbitals ( so 8 electrons ).
27
Isotopes
Two atoms that have the same atomic number but different atomic masses ( so diff. # of neutrons ).
28
Radioactive Isotopes
Isotope atoms w/ an unstable nucleus that radiates particles.
29
Redox reactions
Electrons are transferred from one atom to another. OIL ( Oxidation Is Losing; becomes + ) - RIG (Reduction Is Gaining; becomes - ). *see notes in red spiral for clearer understanding
30
Description of matter
Anything that has mass or takes up space.
31
Combustion chemical reaction
When O2 combines w/ another compound to form H2O and CO2. Exothermic reaction-produces/needs heat. ( A+O2 ----> CO2+ H2O [uses heat] )
32
Synthesis chemical reaction
Two or more simple compounds/atoms combine to form a more complicated compound. ( A + B ----> AB ).
33
Decomposition chemical reaction
Breaking down a complex molecule into simpler compounds/atoms. ( AB ----> A + B ).
34
Single-replacement chemical reaction
When one cation/anion trades places w/ another in the compound. ( AX + B ----> BX + A ).
35
Double-replacement chemical reaction
When the cations or anions of two different molecules trades places; now forming 2 different compounds. ( AB + CD ----> AD + BC ).
36
Acid-base neutralization chemical reaction
Special kind of double-replacement reaction that takes place when and acid and base react w/ each other to form H2O and salt. ( HX + BOH ----> BX + H2O ). ( acid + base -----> salt + water ).
37
Viscosity
Behavior of the flow of fluids described by two properties: - Density of fluids - Newtons law-affected by temp. and pressure
38
Gas Laws
- Volume - Temperature - Pressure - Moles ( amount )
39
VSPER: Non-polar
Charge distribution of electrons is symmetrical ( charges are the same ).
40
VSPER: Polar
Charge distribution of electrons is asymmetrical ( not the same; different charges ).
41
States of Matter
- Solid - Liquid - Gas - Plasma
42
IMF stand for?
Intermolecular Forces. Forces that are between molecules.
43
IMF : Dipole-dipole interaction
Each molecule is polar ( opposite charges ).
44
IMF : Hydrogen bonding
Positively charged hydrogen and electronegative element ( such as Florine, Oxygen, or Nitrogen [ FON] ). Type of dipole-dipole interaction. Is the strongest IMF force.
45
IMF : London Dispersion forces
Weakest IMF. Low boiling point. Mostly gases. Both molecules are non-polar.
46
Van Der Waals bonding
Weakest type of chemical bonding.
47
Water
Solvent in which most other compounds or solutes are dissolved in; aqueous solution.
48
Dehydration synthesis
Reactions where water is lost from the reactants.
49
Hydrolysis
Water is introduced to the reactants to brake the bonds, causing the reactants to be broken into smaller molecules.
50
Energy definition
The ability to do work ( movement of an object by some force ). Two types main : kinetic and potential.
51
Kinetic energy
Energy of motion. | -ex : a moving car has kinetic energy.
52
Potential energy
Energy that matter gains from its arrangement or position. Object has the 'potential' to do work. -ex : a car sitting ( not moving yet ) @ the bottom of a hill facing up; the car has the potential to drive up the hill.
53
Mechanical energy
The sum of kinetic and potential energy. | -ex : a car driving up a hill has both kinetic and potential energy.
54
Freezing point, boiling point, & normal body temperature in Fahrenheit?
- 32 degrees - 212 degrees - 98.6 degrees
55
Freezing point, boiling point, & normal body temperature in Celsius?
- 0 degrees - 100 degrees - 37 degrees
56
Fahrenheit to Celsius formula
F = C x 9 divided by 5 + 32
57
Celsius to Fahrenheit formula
C = ( F - 32 ) x 5 divided by 9
58
Kelvin to Celsius formula
Celsius = Kelvin - 273.15 | - can then take Celsius to Fahrenheit.
59
Cation
Positively charged ion.
60
Anion
Negatively charged ion.
61
The rows in the Periodic Table are called what?
Periods.
62
The columns in the Periodic Table are called what?
Groups. | - think of noble gases.
63
Group I A of the Periodic Table have a _____ charge?
+ 1 charge; 1 valence electron.
64
Group II A of the Periodic Table have a _____ charge?
+ 2 charge; 2 valence electrons.
65
Group III A of the Periodic Table have a _____ charge?
+ 3 charge; 3 valence electrons.
66
Group IV A of the Periodic Table have a _____ charge?
+ 2 or + 4 charge; 4 valence electrons.
67
Group V A of the Periodic Table have a _____ charge?
- 3 charge, 5 valence electrons.
68
Group VI A of the Periodic Table have a _____ charge?
- 2 charge, 6 valence electrons.
69
Group VII A of the Periodic Table have a _____ charge?
- 1 charge, 7 valence electrons.
70
Group VIII A of the Periodic Table have a _____ charge?
``` No charge ( octet is complete ); 8 valence electrons. - Noble gases group. ```
71
What 4 factors increase reaction rate?
- Increase temperature. - Increase surface area. - Introduce catalyst. - Increase concentration.
72
Which material has the smallest specific heat?
Aluminum.
73
Specific Heat
Is the amount of heat required to raise the temperature of 1 gram by 1 degree Celsius.
74
What is the SI unit of energy?
Joule. | - required energy for a force of 1 newton to act over a distance of 1 meter.
75
Which kind of radiation has no charge?
Gamma.
76
Radiation types?
- Gamma - Alpha - Beta
77
Gamma radiation
No charge - sunlight, radio waves - can penetrate human body
78
Alpha radiation
+ 2 charge
79
Beta radiation
- ( neg ) 1 charge | - harmful to human health.
80
What is the mass, in grams, of 1.0 mole of oxygen gas?
32. - 1 mole times 2 oxygen molecules ( oxygen mass is 16 ). - - so 2 x 16 = 32.
81
What is an Empirical Formula?
The smallest expression of a chemical formula; can not be reduced.
82
CH is what type of formula?
Empirical Formula.
83
What is another name for aqueous HI?
Hydriodic acid.
84
What does polyatomic ion mean?
An ion composed of 2 or more elements.
85
What element is not involved in many hydrogen bonds?
Carbon. | - Any element that is not FON ( Florine, Oxygen, or Nitrogen ).

HESI-A2 (2 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions