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Chemistry > Final Semester 1 > Flashcards

Final Semester 1 Flashcards

(64 cards)

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0
Q

Theory

A

Well tested explanation for observation

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1
Q

What are the definitions of organic, inorganic, bio, analytical and physical chemistry?

A

Organic- compounds containing carbon
Inorganic- compound NOT containing carbon
Biochem- processes taking place in organisms
Analytical- composition if matter
Physical- mechanism, rate, and energy transfer that undergoes a change

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2
Q

Independent variable

A

The variable changed in an experiment

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3
Q

Dependent variable

A

Variable observed

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4
Q

Extensive properties

A

A property that depends on the amount of matter in a sample

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5
Q

Intensive properties

A

A property that depends on the type of matter in a sample and not the amount of matter

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6
Q

Weight vs mass

A

Weight- a force that measures the pull of gravity on a given mass
Mass - a measure of the amount of matter that an object contains

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7
Q

Density

A

The ratio of the mass of an object to its volume

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8
Q

Matter

A

Anything that had mass and occupies space

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9
Q

Proton

A

A positively charged subatomic particle

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10
Q

Nucleus

A

The tiny and dense central portion of an atom that is composed of protons and neutrons

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11
Q

Neutron

A

A subatomic partial that is neutral

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12
Q

Atom

A

The smallest part of an element

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13
Q

Isotope

A

Atoms of the same element that have the same atomic number but different atomic masses due to different number of electrons

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14
Q

Atomic mass

A

The weighted average of the masses of the isotopes of an element

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15
Q

Mixture

A

A physical blend of two or more substances that are not chemically bonded

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16
Q

Homogeneous mixture

A

A mixture that is a uniform in composition.; components are evenly distributed and not easily distinguished

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17
Q

Heterogenous mixture

A

A mixture that is not uniform in composition ; components are not evenly distributed throughout the mixture

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18
Q

Vapor

A

Describes the gaseous state of a substance that is generally a liquid or solid at room temperature

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19
Q

Atomic orbital

A

A mathematical expression describing the probability of finding electrons at various locations

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20
Q

Electron configuration

A

The arrangement of electrons of an atom in its ground state into various orbitals around the nuclei of atoms

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21
Q

Photon

A

A quantum of light

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22
Q

Quantum

A

The amount of energy needed to move an electron from one electron from one energy level to another

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23
Q

Electronegativity

A

The ability of an atom to attract electrons when the atoms in a compound

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24
Transition metal
Underneath the step
25
Cation
Any atom with a positive charge
26
Anion
An atom with a negative charge
27
Group
Vertical
28
Period
Horizontal
29
Octet rule
Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas, usually eight valence electrons
30
Ionic bond
One metal and a nonmetal
31
Covalent bond
Both nonmetals
32
Valence electrons
An electron in the highest occupied energy
34
What does a chemical formula represent?
Compounds
35
Differentiate between physical and chemical properties
Physical- quality or condition of a substance that can be observed or measured without charging the substance's composition Chemical- the ability of a substance to undergo a specific chemical change
36
What happens to the energy of an electron when it moves from a lower to a higher energy level?
The elctronn must gain or loose the right amount of energy.
37
Which subatomic particle determines the properties of an element?
The electrons
38
How can you tell the number of valence electrons in an element?
The group number of an element
39
How do elements in group 2A obey the octect rule?
They will lose two valence electrons.
40
What does the atomic mass of an element represent?
A unit of mass equal to 1/12 the mass of a carbon- 12 atom
41
List all of the differences in chemical properties between ionic and covalent compunds.
Ionic- high melting, conduct in water, and soluble with other ionic compounds Covalent- low melting, not very conductive, and soluble with other covalent compunds
42
List the diatomic particles.
H O F Br I N Cl | Hydrogen, Oxygen, Fluorine, Bromine, Iodine, Nitrogen and Chlorine
43
How do cations obey the octect rule versus anions?
A cation loses valence electrons while anions gain.
44
What does it mean if a compound ens in -ate or -ite versuds ide?
Acids: -ate=ic -ite= ous | -ide if there is no polyatomic ion at the end
45
What is a polyatomic ion?
A tightly bound group of atoms that behave as a unnit and has a positive or negative charge.
46
How are ionic compounds generally written?
With using the criss cross method and the elements' charages
47
How are molecular compounds generally written? (covalent compounds)
Using the prefixes but mono does not need to be used in the first element. Bromine Tetraoxide instead of Monobromine Tetraoxide
48
How is the charge of a transition metal generally written in a formula?
After the element there is a roman numeral following that states the charge of the transition metal.
49
What are the prefixes for naming covalent bonds?
``` Mono- 1 Di- 2 Tri-3 Tetra- 4 Penta- 5 Hexa- 6 Hepta- 7 Octa-8 Nona- 9 Deca- 10 ```
50
What is the SI unit for representive particles?
Mole
51
Differentiate between Alpha, Beta, and Gamma particle emission.
Look at sheet
52
What is STP and what is the molar volume of gas at STP?
STP stands for Standard Temperature and Pressure | The molar volume is 1 mol/ 22.4 L or 22.4 L/ 1mol
53
A ca^2+ ion differs from a Ca^0 atom in that the first ion has
Fewer electrons
54
The chemical properties of an atom are related to the number of its
Valence electrons
55
What is the total number of electrons in a cr3+ ion?
21
56
An atom of 226 RN | 88 contains how many protons and electrons
88 protons and 138 electrons
57
An atom that contains 8 protons 8 electrons and 9 neutron a has a mass number of what?
17
58
Give an example of an isotope of carbon
12 C and 13 C | 6. 6
59
The total number of electrons in an atom of phosphorus in ground state is
5
60
What is the total number of electrons in the atom of 59 Co | 27
27
61
How do you get the number of neutrons?
Mass# - atomic #
62
When do you use scientific notation?
When there is a large number with a lot of zeros
63
What does 23,000,000 become in scientific notation?
It becomes 2.3 x10^ 7
64
What does 0.00087 become in scientific notation?
8.7 x10^-4

Chemistry (15 decks)

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