Mid-Term Chapters 1,2,3,19 Review – Flashcards

Always wear goggles or eye protection when conducting an experiment.

1) Tell the teacher (She will tell you if it's safe or not)

2) Sweep up the glass with the dust pan and brush

3) Put it in the glasswear container (NOT the trashcan)

a) wafting

b) 1) hold the substance away from you

2) use your hand and push air from over the beaker to your nose (DO NOT smell directly)

1) Do not reach over the flame

2) Set up all materials before turning it on

3) Wear protective eye glasses and apron

4) DO NOT leave unattended

Tilt the test tube towards a wall (not yourself or others) and slowly move it back and forth over the flame.

1) Eye Wash Station/ Emergency Shower

2) Fire Blanket

3) Fire Extinguisher

4) Chemical Hood

5) First Aid Kit

Pull: the pin

Aim: the hose

Squeeze: the handle

Sweep: from side to side

False.  

Always add acid to water

1) Wash from the nose out to the ear

2) Flood eyes and eyelids with water for 15-20 minutes

3) Keep the eyes forcibly open

STOP, DROP, AND ROLL!!

used as a container and can be heated

used to heat materials

used for heating solids over a Bunsen burner

used to hold test tubes

used for evaporating materials

used as a container of liquids, not a lot of information.

Do not measure with this! 

used to pick up or hold small objects

used to filter liquids and measure

used to grind solids up

used to hold crucible and lid over Bunsen burner

used to measure liquids and has more information

used to hold beakers and other things over the Bunsen burner, 

holds the Bunsen burner and ring

used as a container and can be heated

used to pick up test tubes

used to pick up hot beakers and other apparatuses

used as a lid for the evaporating dish

used to clean test tubes and other apparatuses

used for spreading out the heat of the flame from the Bunsen burner onto other apparatuses

The tip of the inner core

Main gas valve

The air vent, it is adjusted by screwing the burner tube up and down

the study of compostition, matter, structure, and of changes that occur in matter (chemical reactions)

anything that has mass and occupies space

the smallest distinctive units in a sample of matter

larger units in which 2 or more atoms are joined

types of atoms and the relative proportions of the different atoms in a sample of matter

a characeristic displayed by a sample of matter without undergoing any change in its composition

no change in the substance involved, how it occurs

ex: color, odor, taste, boiling/melting point, physical state, density, solubility, electrical conductivity 

characteristic displayed by a sample of matter as it undergoes a change in its composition

substances are changed, NEW transformation

ex: burn, rot, rust, decompose, ferment, explode, corrode, reactivity, flammability

a sample of matter usually undergoes noticeable change at the macroscopic level but no change in its composition

(aka CHEMICAL REACTION) a sample of matter undergoes a change in composition and/ or change in the structure of its molecules

a type of matter that has a definite (fixed) composition that does not vary from one sample of a substance to another

a substance that cannot be broken down into other simpler substances by chemical reactions

a substance made up of atoms of 2 or more elements, with teh different kinds of atoms combined in fixed proportions

a 1 or 2 letter designation to use symbols that derived from the name of the element

has no fixed composition, it's composition may vary over a broad range

(aka SOLUTION) a mixture that has the same composition and properties throughout

varies in composition and/or properties from 1 part of the mixture to another

a tenative explanation or prediction concerning some phenomenom, must be a guess that can be tested

when scientists test a hypothesis through carefully controlled procedures

the facts obtained through careful observation and measurements made during an experiment

patterns that have been identified in large collections of data and summerized

provides explanations of observed natural phenomena and predictions that can be tested by further experiments

the amount of matter that a substance contains

what humans can see, large --> macro

actual particles (atoms, etc) small --> micro

definite

definite

definite

indefinite

indefinite

indefinite

DIFFERENT

separates a solid from a liquid

ex: sand and water lab

separates dissolved solids from liquids

ex: salt and water lab

separation of two liquids

separates mixtures as the solvent travels across the paper by capillary action, the components of the mixture separate, the components of the mixture that are most soluble in the solvent and least attracted to the paper travel the farthest

a) a stationary phase (filter paper)

b) a liquid (mobile) phase (solvent: water) 

Physical Property

Physical Property

Chemical Property

Physical Property

Physical Property 

Chemical Property

Physical Property

Chemical Property

Physical Property

Homogeneous element

Homogeneous compound

Heterogeneous, compound

Homogeneous, compound

Homogeneous, element

Heterogeneous, compound

is a statement of fact, based on what you detect by your senses

is your judgement or opinion about what you have observed

is an observation that involves a measurement

is a general description and does not involve a measurement

a judgement based on the results of an experiment

number between 1-10

a positive or negative integer in scientific notation which shows the power of the coefficient

1) if decimal is moved to the right the exponent is negative

2) if decimal is moved to the left the exponent is positive

Addition

ex: (6.7 x 10³) x (5.2 x 10⁴) = 34.84 x 10⁷

correct sci. notation = 3.484 x 10⁸

Subtract

ex: (2.3 x 10²) x (6.6 x 10⁵) = 15.18 x 10^-3

correct sci. notation = 1.518 x 10^-2

the exponents must be the same for all numbers involved

(2.3 x 10³) + (3.5 x 10³)

.23 x 10³ + 3.5 x 10³ = 3.73 x 10³

meter (m)

kilogram (kg)

second (s)

Kelvin (K) 

mole (mol) 

Ampere (A)

combining fundamental units

l x w x h= units³= (mL)

mass / volume = grams / cm³ = g / mL

kg x m² / s² = Joule

2.37 x 10³

4.5 x 10^-5

10⁹

10³

10^-6

1.35 x 10¹²

7.7 x 10⁵

4.183 x 10³

Metric System (SI)

grams

liters

meters

10³ 10² 10¹ base 10^-1 10^-2 10^-3

kilo: one thousand times

hecto

deca

deci

centi: one one hundredth 

milli: one one thousandth

an indication of heat energy

the transfer of energy from an object at higher temperature to an object at a lower temperature

Fahrenheit

Celsius

Kelvin

f.p. 0

b.p. 100

f.p. 32

b.p. 212

f.p. 273

b.p. 373

t_K = t_C + 273

t_C = t_K - 273

degree of agreement among several measurements of the same quantity (reproductibility)

**depends on more than 1 measurement (3x)

agreement of a particular value with the true value

**often depends on the quality of the measuring (calibration) instrument**

*the accepted value is predetermined*

definite and will always be the same and are read directly from the instrument

estimated and may vary

recorded digits from a measurement which include all of the digits that are certain and a last digit that is estimated

ONLY when dealing with measured quantities

NO counting numbers

NO equivalent statements

nonzero digits 1-9

captive zeros (205)

trailing zeros with a decimal (5,000.)

coefficients in scientific notation

trailing zeros without a decimal

leading zeros (0.0003)

NEVER

a physical property of a pure substance that depends on the composition of the substance, not the amount

Mass (g) / Volume (cm³ or mL)

** 1 cm³ = 1 mL**

it determines if a material feels "light" or "heavy" and when it will float (it will float on a material that has a greater density)

g/cm³ or g/mL

a way for scientists to express how far off a laboratory value is from the commonly accepted value

experimental value determined based on lab work

predetermined true value

% Error = I Accepted- Experimental I x 100

Accepted value

1) multiplying a quantity by one does not change the quantity

2) the same quantity (or unit) in both the numerator and denominator of the fraction will cancel

2 different values for the same amount in English metric

ex: Mass 453.6 = 1 lb.

to change

M = D x V

V = M / D

pie x r² x h =V

use the one that cancels the unit we do not want and leaves the unit we do want

Greek philosopher (400 B.C) stated matter was composed of small particles

Greek Philosopher (400 B.C.) used the term "atomos" for particles

Greek Philopsopher (400 B.C.) disagreed with Democritus and Leucippos and stated that matter was composed of 4 elements: wind (air), earth, fire, and water

wrong

2000 years (1400's-1500's)

tried turning regular substances into gold

provided valuable information on acids

(FATHER OF CHEMISTRY) (1743-1794)

explained combustion, supported and verified the Law of Conservation of Mass

the total mass remains constant during a chemical reaction

(1754-1826)

Law of Definite Proportions

(aka Law of Constant Composition) 

all samples of a compound have the same composition, that is, all samples have all the same proportions, by mass, of the elements present

(1766-1844)

Law of Multiple Proportions

Atomic Theory

in 2 or more compounds of the same 2 elements, the masses of 1 element that combine with a fixed mass of the 2nd element are in the ratio of small whole numbers

small, densely packed nucleus which contains protons and neutrons; these subatomic particles provide the mass of the atom

the nucleus is then surrounded by electrons, electrons are not considered when calculating the mass of the atom

charge = +

+ charge = - charge

# protons = # electrons

Atomic number (# protons)

*this remains constant for a given element*

it identifies the element on the periodic table (counting number) 

# protons + # neutrons = MASS NUMBER

to express the atomic structure for a given type of atom

shows the atomic number (Z) and the mass number (a)

1) Each element is made up of tiny, indivisible particles

2) Atoms of a given element are not always identical

3) Chemical compounds are formed when atoms of different elements combine with each other.  A given compound always has the same relative numbers + types of atoms. -Law of Definite Proportions

4) Chemical reacitons involve reorganization of the atoms- changes in the way they are bound together- the atoms themselves are not changed in a chemical reaction. - Law of Conservation of Mass

1) Atoms are not indivisible 

-made up of protons, neutrons, and electrons (sub-atomic)

2) Atoms of a given element are not always identical

-Isotopes cause variations (same # of protons dif # of neutrons)

the mass of each individual isotope of each element is determined in comparison to this standard (carbon-12 as the standard at 12 amu) using a mass spectrometer

#p + #n

specific to individual isotopes

structural

whole number

weighted average

decimal

applies for ALL Isoptopes

elemental

percent abundance

ALL

1) the relative mass for each isotope

2) the percentage occurance for each isotope

-the result is an averaged mass for all particles in a sample

6:02 am - 6:02 pm on October 23

(1803-1895)

arranged elements using Atomic mass and physical/ chemical properties

predicted the existence of scandium, gallium, and germanium

Metals and Non-metals

solids (except Hg)

conductors of heat and electricity

malleable and ductile 

lustrous

*tend to lose electrons to form IONS whith a positive charge called a CATION*

solids, liquids (Br) or Gases

nonconductors

brittle

non lustrous/ dull

*tend to gain electrons to form IONS with a negative charge called ANIONS*

(semimetals)

elements display properties between metals and non-metals

*semiconductors*

In Periods and Groups

horizontal rows

verticle columns

IA

very reactive

+1 ion

IIA

reactive

+2 ions

Nonmetals

VII A

very reactive

-1 ion

exist as diatomic molecules

Nonmetals

VIII A 

UNREACTIVE

exist as monatomic gases

form a stair-step division between metals and non-metals

can form more than one possible ion with a + charge

radioactive and synthetic elements

A Groups: representative elements

B Groups: transition metals

ionic bonds

covalent bond (molecular composition)

when atoms share electrons

this structure results in a new particle: the molecule

solids, liquids, or gasses

generally low or very low melting points

variable boiling points

nonconductors

F₂, Cl₂, Br₂, I₂

H₂, N₂, O₂

P₄, S₈

when atoms gain or lose electrons to form changed particles

when a neutral atom gains an electron

has a negative charge

when a neutral atom losses and electron

has a positive charge

the structure that results from the attraction between anions and cations form an ionic bond

occur only as solids

high melting points

very high boiling points

nonconductors as solids

can conduct electricity when melted or when dissolved in a solution

when we name binary molecular compounds we use PREFIXES to specify how many atoms of each element are present

second element ends in -ide

NO prefix is used when there is only one atom of the first element

use the prefixes to tell how many atoms of that element

determine the symbols/ formulas and charge

determine charges

use subscripts to balance the charges

NO CHARGES in final formula 

CaCl ---> CaCl₂

NH₄NO₃ 

Mg OH ---> Mg(OH)₂

ionic compounds / salts that have water molecules as part of their solid crystalline structure (special category of ionic compounds

copper II sulfate pentahydrate 1:5

1 formula unit for salt : # H₂O molecules

as an ACID

as a BASE

Acids: (H is the first element) binary (H+ nonmetal)

uses prefix hydro-

for second element use ic- ending

Base: Ternary (H+ polyatomic ion)

NO HYDRO-

use root name of polyatomic ion and change -ate to -ic

change -ite to -ous

a nucleus with a specified number of protons and neutrons and a specified energy

(a) consists of 2 protons and 2 neutrons; it is identical to a doubly ionized helium ion He²⁺

(B) an electron, is emitted by the nucleus of certain radioactive atoms as they decay

(Y) highly penatrating form of electromagnetic radiation

particles having the same mass as electrons by carrying a charge of 1+

a process in which the nucleus absorbs an electron from an inner electron shell (1 or 2) 

protons and neutrons collectively

the time required for one-half of a statistically large numbr of radioactive material to decay due to transmutation/ radioactive decay

a series of radioactive decays beginning with a long lived radioactive nucleotide and ending with a non radioactive one

(1852- 1908)

accidental discovery of energy given off naturally by uranium salts

worked with Becquerel and coined "radioactivity"

nuclei undergo changes in order to go from an unstable isotope (radioisotope) to a stable isotope

large amounts of energy are involved

process in which the nucleus undergoes decomposition to form a different nucleus

energy/particles released in the process of radioactive decay

subtact a He ion from the radioactive isotope

*conservation of nucleons*

add an electron to the radioactive isotope

high energy electromagnetic radiation

can be emitted by alpha or beta particles 

no particles of its own, it's made of photons

no real change in the nucleus

(ATOMIC BOMB)

process of changing one element to another due to radioactive decay

a handheld device that is used to detect radioactive minerals and inspect equipment in nuclear and x-ray facilities

a personal exposure monitoring device worn by individuals whose work exposes them to ionizing radiation.  badges are collected on a regular basis to check for levels of exposure

a technique used to date materials such as rocks in geologic time, remains from living organisms, and artifacts from past societies

used in medicine and research to tag atoms in molecules so that they can be traced and monitored in chemical reactions and metabolic pathways.  

Also used in diagnostic procedures such as PET and CT scans and in medical treatment of various cancers

(NUCLEAR MEDICINE)

splitting atoms

nuclear reactions

combining atoms

ex:the sun

the number equal to the number of carbon atoms in exactly 12 grams of C-12

mass of 1 mole of an element or of a compound using element masses, given in the periodic table, expressed in grams

a sample of an element with a mass in grams equal to the element's average atomic mass (from P.T) will contain 1 mole of atoms

compounds are defined by their chemical formula

we use the information to calculate the molar mass of a compound