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60 Cards in this Set

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Label this element and the meanings of the values.
29
Cu
63.546
29=atomic number
Cu=element=copper
63-546=atomic mass
Define the meaning of the letters.
A
X
Z
A=mass number
Z=atomic number
X=element symbol
What is the atomic number?
What is the mass number?
Atomic #=the number of protons, defines the element, different elements have different # of protons.
Mass #= A(the # of protons)+ number of neutrons
What element group is group 1A?
alkali metals
Name all the elements that are alkali metals along with their abrreviations.
Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Cesium (Cs), Francium (Fr)
What element group is group 2A?
alkaline earth metals
Name all of the elements that are alkaline earth metals along with their abrreviations.
Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba) and Radium (Ra)
What element group is group 7A?
halogens
Name all of the elements that are halogens along with their abbreviations.
Flourine (F), Chlorine (Cl), Bormine (Br), Iodine (I), and Astatine (At)
What element group is group 8A?
noble gases
Name all of the elements that are noble gases along with their abbreviations.
Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xeon (Xe) and Radon (Rn)
What is a metal?
a good conductor of heat and electricity
What is a nonmetal?
a poor conductor of heat and electricity
What is a metalloid?
has properties that are intermediate between those of metals and nonmetals.
What are the atomic numbers of the elements that are metalloids and separate the metals and nonmetals?
5 , 14, 32, 33, 51, 52, 84, 85, 116, 117
What is one nonmetal that is one the side of the periodic table of the metals?
hydrogen-atomic #=1
Draw the classification of matter tree.
the classification of matter tree
What is a compound?
a substance composed of atoms of 2 or more elements chemically united in fixed proportions.
What are the three states of matter?
solid, liquid and gas`
What is a mixture?
a combination of 2 or more substances in which the substances retain their distinct identities.
What is a homogenous mixture?
Give an example.
the composition of the mixture is the same throughout.
ex. sugar dissolved in water
What is a heterogeneous mixture?
Give an example.
The composition of the mixture is not uniform.
ex. sand in iron fillings.
What is an element?
a substance that cannot be separated into simpler substances by chemical means.
Classify each of the following as an element, a compound, a homogeneous mixture, or a heterogeneous mixture.
a)water
b)salt water
c)oxygen gas
d)air
e)gasoline
f)tomato juice
a)water-compound (H20=2 elements combined)
b)salt water-homogeneous mixture( 2 compounds mixed together, salt dissolves)
c)oxygen gas-element
d)air-homogeneous mixture-(they do not react together)
e)gasoline-homogeneous mixture-all soluble to one another
f)tomato juice-heterogeneous mixture-can see particles
What is a substance?
a form of matter that had a definite (constant) composition & distinct properties
What is matter?
anything that occupies space and has mass
What is a physical change?
Give an example.
a change that does not alter the composition or idenitity of a substance
ex. ice melting (still H20, just stronger bonds when ice)
sugar dissolving in water
What is a chemical change?
Give an example.
a change that alters the composition or identity of the substance(s) involved.
ex. hydrogen burns in air to form water
What is an extensive property?
Give examples.
the property of a material depends on how much matter is being considered.
ex. mass, length, volume
What is an intensive property?
Give examples.
the property of a material that does not depend upon how much matter is being considered.
ex. temperature, color, density
Do the following statements describe chemical and physical properties?
a)irons tends to rust
b)fertilizers help to increase agricultural production
c)water boils below 100 degrees celsius
d)lead is denser than aluminum
e)lithium reacts violently with water
a)irons tends to rust-chemical
b)fertilizers help to increase agricultural production-chemical
c)water boils below 100 degrees celsius on top of a mountain-physical
d)lead is denser than aluminum-physical
e)lithium reacts vilently with water-chemical
Name the rules to determine how many significant figures there are in a number.
1.any number not zero
2. zeros between non-zero digits
3. zeros to the left are non-significant
4. if there are zeros that follow any number greater than 1, they they are significant
5. for nondecimal numbers do scientific notation to determine amount of sig figs
What are the SI base units and there symbols for:
a)length
b)mass
c)time
d)electrical current
e)temperature
f)amount of substance
g)luminous intensity
a)length-meter-(m)
b)mass-kilogram-(kg)
c)time-second-(s)
d)electrical current-ampere-(A)
e)temperature-kelvin-(K)
f-amount of substance-mole-(mol)
g-luminous intensity-candela-(cd)
What are the meanings and symbols for these prefixes used with SI units:
1)tera
2)giga
3)mega
4)kilo
5)deci
6)centi
7)milli
8)micro
9)nano
10)pico
1)tera-1x10^12(base unit)
2)giga-1x10^9(base unit)
3)mega-1x10^6(base unit)
4)kilo-1x10^3(base unit)
5)deci-1x10^-1(base unit)
6)centi-1x10^-2(base unit)
7)milli-1x10^-3(base unit)
8)micro-1x10^-6(base unit)
9)nano-1x10^-9(base unit)
10)pico-1x10^-12(base unit)
For volume determine how much 1cm cubed would equal in meters, and how much 1dm cubed would equal in meters.
1cm cubed=(1x10^-2m)^3=1x10^-6m cubed
1dm cubed=(1x10^-1m)^3=1x10^-3m cubed
Another common unit for volume is liters. How many cm cubed does 1 Liter equal, how many mL does 1 Liter equal, and how many dm cubed does 1 Liter equal
1 L= 1000 cm cubed
1 L= 1000 mL
1 L= 1 dm cubed

This determines that 1mL=1 cm cubed and that 1 dm cubed=1 L
What is the volume in units of m^3 of 3.2 cm^3?
3.2x10^-6 m cubed
What is the equation for density?
density=mass
-----
Volume
Calculate the density of mercury if 1.00x10^2g occupies a volume of 7.35cm^3.
D=1.00x10^2
--------- = (13.6g/cm^3)
7.35cm^3
What are the conversion formulas for degrees Farenheit to degrees Celsius, degrees Celsius to degrees Farenheit, and degrees Celsius to Kelvins.
*C=(*F-32*F)x 5*C
---
9*F
*F= 9*F (*C) + 32*F
---
5*C
K= (*C + 273.15*C)
Perform the following termperature conversions:
a)37*C (normal body temperature) to *F
b)113*C (melting point of pure sulfur) to K
c)Convert 172.9*F to *C
a)99*F
b)386K
c)
What is the number of significant figures in each of the following measured quanitites?
a)1282 kg
b)0.00296 s
c)8.070 mm
d)120 mL
e) 1.2 x10^1 mL
a) 4
b) 3
c) 4
d) 2
e) 2
What are the guidelines for the mathematical problems for significant figures?
a) addition and substaction
b) multiplication and division
a)the answer canno have more digits to the right of the decimal point than either of the original numbers
b)limited by the amount of sig figs according to the original numbers with the smallest # of sig figs
Express the answers to the following calculations with the correct number of sig figs.
a) 5.6792 + 0.6 + 4.33
b) 3.70 - 2.9133
a) 10.6
b) 7.9 x 10^-1
Express the answers to the following calculations with the correct number of sig figs.
a)4.51 x 3.6666
b)3.53/2.0
a)16.5
b)1.8
Express the answers to the following calculations with the correct number of sig figs.
a) 320.55 - (5104.5/2.3)
b) (1.0045x20,000.0)+ (2813x12)
c) 863x [1255-(3.45x108)]
a)1.9x10^3
b)5.4x10^4
c)7.62x10I^5
What is the difference between accuracy and precision?
accuracy is how close a measurement is to the true value of the quantity that was measured.
precision refers to how closely 2 or more measurements of the same quantity agree with one another.
Solves these problems. Hint=1km=0.6215mi
a) You want to run 5K race. Assume that the distance of the 5K race is measured to the preciseness of 5.0km.What is the distance in units of miles?
b) The distances between your home and school is 10.2 miles. What is the distance in units of km?
a)3.1 mi.
b)16.4 km
Show the formula for conversion of units.
given unitx desired unit= desired
------------
given unit
Solve these problems. Hint=1 lb=453.6g
a)What is the weight of a 117 lb person in units of kg?
b)The density of copper is 8.96g/cm^3. what is the density in units of kg/m^3.
a)53.1kg
b)8.96 x 10^3 kg/m^3
Describe a summary of John Dalton's theory of atoms.
1.Elements are composed of extremely small particles called atoms. All atoms of a given element are identical, having the same size, mass, and chemical properties. The atoms of one element are different from the atoms of all other elements.
2)Compounds are composed of atoms of more than one element. In any compound the ratio of the numbers of atoms of any two of the elements present is either an integer or a simple fraction.
3. a chemical reaction involves only the separation, combination, or rearrangement of atoms;it does not result in their creation or destruction
HOw do you find the number of neutrons in a neutral atoms?
Use the number of protons.
Fill in the table
The table filled in
Give the charges for each of the following elements:
a)Li b)Na c)K d)Rb e)Cs f)Mg g)Ca
h)Sr i)Ba j)Cr k)Mn l)Fe m)Co n)Ni o)Cu p)Zn q)Ag r)Cd s)Hg t)Al u)C v)Sn w)Pb x)N y)P z)O
A)S B)Se C)Te D)F E)Cl F)Br G)I
The charges for elements
memorize the following cations and anions
memorize the following cations and anions
memorize the following monoatomic anions and their positions
memorize
fill in the following table
fill in the following table
What are the prefixes for the following numbers
1.
2.
3.
4.
5.
6
7
8.
9
10
memorize
Make a flow chart for naming compounds
the flow chart for naming compounds
fill in the following table for naming compounds
naming compounds