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Chemistry > Final Semester 1 > Flashcards

Final Semester 1 Flashcards

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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
Q

Transition metal

A

Underneath the step

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25
Q

Cation

A

Any atom with a positive charge

26
Q

Anion

A

An atom with a negative charge

27
Q

Group

A

Vertical

28
Q

Period

A

Horizontal

29
Q

Octet rule

A

Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas, usually eight valence electrons

30
Q

Ionic bond

A

One metal and a nonmetal

31
Q

Covalent bond

A

Both nonmetals

32
Q

Valence electrons

A

An electron in the highest occupied energy

34
Q

What does a chemical formula represent?

A

Compounds

35
Q

Differentiate between physical and chemical properties

A

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
Q

What happens to the energy of an electron when it moves from a lower to a higher energy level?

A

The elctronn must gain or loose the right amount of energy.

37
Q

Which subatomic particle determines the properties of an element?

A

The electrons

38
Q

How can you tell the number of valence electrons in an element?

A

The group number of an element

39
Q

How do elements in group 2A obey the octect rule?

A

They will lose two valence electrons.

40
Q

What does the atomic mass of an element represent?

A

A unit of mass equal to 1/12 the mass of a carbon- 12 atom

41
Q

List all of the differences in chemical properties between ionic and covalent compunds.

A

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
Q

List the diatomic particles.

A

H O F Br I N Cl

Hydrogen, Oxygen, Fluorine, Bromine, Iodine, Nitrogen and Chlorine

43
Q

How do cations obey the octect rule versus anions?

A

A cation loses valence electrons while anions gain.

44
Q

What does it mean if a compound ens in -ate or -ite versuds ide?

A

Acids: -ate=ic -ite= ous

-ide if there is no polyatomic ion at the end

45
Q

What is a polyatomic ion?

A

A tightly bound group of atoms that behave as a unnit and has a positive or negative charge.

46
Q

How are ionic compounds generally written?

A

With using the criss cross method and the elements’ charages

47
Q

How are molecular compounds generally written? (covalent compounds)

A

Using the prefixes but mono does not need to be used in the first element. Bromine Tetraoxide instead of Monobromine Tetraoxide

48
Q

How is the charge of a transition metal generally written in a formula?

A

After the element there is a roman numeral following that states the charge of the transition metal.

49
Q

What are the prefixes for naming covalent bonds?

A 
Mono- 1
Di- 2
Tri-3 
Tetra- 4
Penta- 5 
Hexa- 6
Hepta- 7
Octa-8
Nona- 9 
Deca- 10
50
Q

What is the SI unit for representive particles?

A

Mole

51
Q

Differentiate between Alpha, Beta, and Gamma particle emission.

A

Look at sheet

52
Q

What is STP and what is the molar volume of gas at STP?

A

STP stands for Standard Temperature and Pressure

The molar volume is 1 mol/ 22.4 L or 22.4 L/ 1mol

53
Q

A ca^2+ ion differs from a Ca^0 atom in that the first ion has

A

Fewer electrons

54
Q

The chemical properties of an atom are related to the number of its

A

Valence electrons

55
Q

What is the total number of electrons in a cr3+ ion?

A

21

56
Q

An atom of 226 RN

88 contains how many protons and electrons

A

88 protons and 138 electrons

57
Q

An atom that contains 8 protons 8 electrons and 9 neutron a has a mass number of what?

A

17

58
Q

Give an example of an isotope of carbon

A

12 C and 13 C

6. 6

59
Q

The total number of electrons in an atom of phosphorus in ground state is

A

5

60
Q

What is the total number of electrons in the atom of 59 Co

27

A

27

61
Q

How do you get the number of neutrons?

A

Mass# - atomic #

62
Q

When do you use scientific notation?

A

When there is a large number with a lot of zeros

63
Q

What does 23,000,000 become in scientific notation?

A

It becomes 2.3 x10^ 7

64
Q

What does 0.00087 become in scientific notation?

A

8.7 x10^-4

Chemistry (15 decks)

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