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CHEM 501 > Module 1 & 2 > Flashcards

Module 1 & 2 Flashcards

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1
Q

chemistry is

A

the study of matter, its chemical and physical properties, the chemical and physical changes it undergoes, and the energy changes that accompany those processes

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2
Q

matter is

A

anything that has mass and occupies space

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3
Q

matter gains and loses ____ as it undergoes ___

A

energy; change

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4
Q

The scientific method is

A

a systematic approach to the discovery of new information

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5
Q

Characteristics of the scientific method include:

A

observation of a phenomenon; formulation of a question concerning the observation; presentation of a hypothesis; experimentation, with the collection and analysis of data and results in an attempt to support or disprove a hypothesis; ultimate goal of process is to form a theory supported by extensive testing

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6
Q

a scientific law is

A

the summary of a large quantity of information supporting a theory or hypothesis

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7
Q

pure substances of matter can be subdivided into what two groups?

A

elements or compounds

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8
Q

mixtures can be subdivided into what two groups?

A

homogeneous mixtures or heterogeneous mixtures

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9
Q

properties of matter can be classified as what two things?

A

physical property and chemical property

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10
Q

a physical property is

A

observed without changing the composition of matter

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11
Q

a chemical property is

A

observed as the matter is converted to a new substance

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12
Q

properties can be classified into what two categories?

A

intensive and extensive

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13
Q

intensive property is

A

a property that does not depend on the quantity of matter

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14
Q

extensive property is

A

a property that does depend on the quantity of matter

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15
Q

Why does the metric system have a advantage over the English system?

A

metric units are systematically related to each other by powers of ten

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16
Q

mass is…

A

a measure of the quantity of matter

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17
Q

Weight is

A

the force of gravity on an object

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18
Q

the metric unit for mass is ____; a common English mass unit is the ____

A

gram; pound

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19
Q

length is

A

the distance between two points

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20
Q

volume is

A

the space occupied by an object

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21
Q

the metric unit of time is the___

A

second

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22
Q

significant figures are

A

all digits in a measurement known with certainty plus one uncertain digit

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23
Q

what is scientific notation?

A

a way to express a number as a power of ten

24
Q

temperature is

A

the degree of hotness of an object

25
Q

energy is

A

the ability to do work

26
Q

energy is categorized as ___ energy and ____ energy

A

kinetic and potential

27
Q

concentration is

A

a measure of the amount of a substance contained in a specified amount of a mixture

28
Q

density is

A

the ratio of mass to volume and is an intensive property; typically reported as g/mL or g/cm3

29
Q

specific gravity is

A

the ratio of the density of an object to the density of pure water at 4 degrees C; numerically equal to density but without units

30
Q

What are the 6 postulates of Daltons atomic theory?

A

all matter consists of tiny particles called atoms; an atom cannot be created, divided, destroyed, or converted to any other type of atom; atoms of a particular element have identical properties; atoms of different elements have different properties; atoms of different elements combine in simple whole-number ratios to produce compounds (stable combinations of atoms);

31
Q

spectroscopy

A

information obtained from the absorption or emission of light by atoms that yield valuable insight into structure of an atom

32
Q

electromagnetic radiation travels in ___ from a source; the most recognizable source is the ___

A

waves; sun

33
Q

the speed of light is notated as

A

3.0 x 10-to-the-8th power m/s

34
Q

electromagnetic spectrum

A

a collection of all electromagnetic radiation, including each of the different wavelengths

35
Q

what is electron density?

A

the proportion (density) to the probability of finding the electron at any point in time

36
Q

the periodic law is…

A

embodied by Mendeleev’s statement which states “the elements, if arranged according to their atomic weights (masses), show a distinct periodicity (regular variation) of their properties”

37
Q

Describe a common property of metals? Nonmetals?

A

Metals tend to lose electrons while nonmetal tend to gain them

38
Q

What are principal energy levels?

A

regions where electrons may be found and in which integral values are designated n = 1, n = 2, n=3, etc.; related to the average distance from the nucleus; n = 1 level is the closest to the nucleus

39
Q

The maximum number of electrons that a principal energy level can hold is equal to what?

A

2(n) to the 2nd power

40
Q

Only one ___ orbital can be found in any ___ orbital

A

s; n

41
Q

Which orbitals are important in determining the properties of the transition metals?

A

d orbitals

42
Q

what are paired electrons?

A

two electrons in one orbital that possess opposite spins ; their number and arrangement within an atom are responsible for magnetic properties of elements

43
Q

no more than __ electrons can be placed in any orbital; each principle energy level (n) can contain only ___ subshells

A

2; n

44
Q

what is the aufbau principle?

A

electrons fill the lowest energy orbital that is available

45
Q

What is the electron capacity of the s orbital? p? d?

A

2; 6; 10

46
Q

what is isoelectric?

A

an ion that has the same electron configuration as its nearest noble gas, making it stable

47
Q

Transition and representative metals tend to form ___ by losing electrons

A

cation

48
Q

nonmetallic elements tend to form ___ by gain electrons

A

anions

49
Q

what is electron affinity?

A

the potential to gain electrons, or the energy change when a single electron is added to an isolated atom; large electron affinity mans a large release of energy indicating more electrons equal a more stable atom

50
Q

ionization energy is

A

the energy required to remove an electron from an isolated atom; decreases down a group; increases across a period; highest for noble gases

51
Q

electron affinities generally ___ down a ___ and ___ across a ____

A

decrease; group; increase; period

52
Q

Which of the following properties of matter is not considered to be an intensive property but rather is best understood as an extensive property?

A

mass

53
Q

What are the correct expressions when the following numbers are put into scientific notation? 113.7789; 0.0003885; 5.229

A

1.137789 x 102and 3.885 x 10-4and 5.229

54
Q

Which of the following atoms or ions does not contain a full octet of electrons in its outmost energy level? Magnesium is in Group IIA; sulfur is in Group VIA; bromine is in Group VIIA; Argon is in Group VIIIA.

A

S

55
Q

Which of the following is the correct electron configuration for a neutral atom of chlorine (Cl), atomic number 17? Chlorine is located in Group VIIA and period 3 of the periodic table.

A

1s2, 2s2, 2p6, 3s2, 3p5

56
Q

Which of the following elements is not classified as a metal in the periodic table?

A

selenium

CHEM 501 (13 decks)

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