Basics

Question 1

What are the units of measurement for the following in the metric system?:
Length
Volume
Mass
Temp
Time

Answer 1

Length: meter
Volume: liter
Mass: gram
Temp: degree Celsius 
Time: second

Question 2

What are the units of measurement for the following in SI?:
Length
Volume
Mass
Temp
Time

Answer 2

Length: meter
Volume: cubic meter
Mass: kilogram
Temp: kelvin (K)
Time: second

Question 3

Length:
1m = how many feet?
1m = how many yards?
1 inch = how many cm
1 inch = how many mm?

Answer 3

Length: 
1m = 3.37 feet
1m = 1.09 yard
2.5cm 
25mm

Question 4

what is volume?
1L = how many qt?
how many L are in 1m^3

Answer 4

The amount of space a substance occupies
1L = 1.06qt
1000 L

Question 5

1. what is matter?
2. what is a pure substance?
3. what is an element?
4. what is a compound?

Answer 5

1. anything that has mass and occupies space
2. matter that has a fixed or definite composition
3. the simplist type of pure substance composed of only one type of material ie: silver
4. a pure substance that is composed of two or more elements

Question 6

how can compounds be broken down?

Answer 6

by chemical processes. Cannot be broken down by physical processes such as boiling.

Question 7

1. what is a mixture?
2. what is homogenous?
3. what is heterogenous?

Answer 7

1. two or more substances are mixed, but not chemically combined (therefore can be separated by physical processes).
2. aka a solution. Composition is uniform throughout
3. not a uniform composition. ie: oil and water

Question 8

1. What are physical properties?
2. What are physical changes?
3. What are chemical properties?
4. What is a chemical change?

Answer 8

1. characteristics that can be observed or described w/o affecting the identity of the substance.
2. when state, size, or appearance changes, but composition remains the same. ie: water turns to vapor or ice.
3. they describe the ability of a substance to change into a new substance.
4. when original substance converts into one or more new substances. ie: when iron reacts with oxygen to form rust.

Question 9

1. What is the conversion formula for F to C?
2. What is the conversion formula for C to F?
3. At what temp does water freeze in Kelvin?
4. What is the conversion from C to K?

Answer 9

1. Temp in F = 1.8(Temp in C)+32
2. Temp in C = Temp in F - 32/1.8
3. Freezes at 273K
4. Temp in K + 271

Question 10

1. What is the SI unit for energy?

2. How many J = 1 cal?

Answer 10

1. Joule

2. 4.184 J = 1 cal

Question 11

1. What is specific heat?
2. What is the formula for specific heat (aka the heat equation)?
3. Water has a specific heat of …… is this considered a low or high specific heat? How does this benefit our planet?

Answer 11

1. for any given substance it is the amount of heat needed to raise the temp of 1g by 1 C ( written as delta T)
2. heat = mass x temp change x SH
3. water requires 1 cal or 4.184 J to raise 1g by 1C. This is a high specific heat. This high SH keeps water temps more moderate through summer and winter.

Question 12

1. What is the heat of fusion?

2. what is the formula for heat of fusion?

Answer 12

1. The energy that must be added to convert 1g of solid to liquid at the melting point. For example, water needs 80cal or 334J per gram to tip from solid to liquid. This is also true in reverse. To tip from liquid to solid, 80 cal or 334 J must be removed when at its freezing point.
2. heat = mass x heat of fusion

Question 13

1. What is sublimation?

2. What is deposition?

Answer 13

1. when the particles on the surface of a solid change directly to a gas without temperature change and without going through a liquid state. Ex: dry ice
2. Exact opposite of sublimation. In deposition, gas particles change directly to a solid. Ex: when water vapor turns to ice. Hoar frost

Question 14

Precision vs accuracy

Answer 14

Precision: how close measures are together each time.

Accuracy: how close measured are to the true value.

Question 15

How to give answers when multiplying or dividing

Answer 15

Answer to the least number of SFS

Question 16

How to answer when adding and subtracting decimals

Answer 16

Answer to least decimal place.

Question 17

Kilo=
Mega=
Giga=
Tera=

Answer 17

k 1000 = 10^3
M 1 000 000 = 10^6
G 1 000 000 000 = 10^9
T 1 000 000 000 000 = 10^12

Question 18

Deci = 
Centi = 
Milli =
Micro = 
Nano = 
Pico =

Answer 18

d = 0.1 = 10^-1
c = 0.01 = 10^-2
m = 0.001 = 10^ -3
mc = 0.000 001 = 10^-6
n = 0.000 000 001 = 10^-9
p= 0.000 000 000 001 = 10^-12

Question 19

1. Each horizontal row in the periodic table is a ……….. .
2. There are how many periods?
3. Name the first element from each period (row)

Answer 19

1. period
2. 7
3. H hydrogen, Li litheum, Na sodium, K potassium, Rb rubidium, Cs cesium, Fr francium

Question 20

1. Each vertical column contains a ……….. .
2. Group numbers are located where?
3. what are group 1A to 8A
4. in the center of the periodic table there is a block of elements known as ………… ……….. . What letter is assigned to their group?
5. What are the inner transition members?

Answer 20

1. Group or family
2. at the top of each column
3. representative elements
4. transitional elements. B
5. Lanthanides and actinides. They are part of periods 6 & 7, but placed at bottom of page so table can fit on one page

Question 21

1. What is the special name for group 1A? Is H part of this group?
2. What is the special name for group 2A?
3. What is the special name for group 7A?
4. What is the special name for group 8A?

Answer 21

1. Alkali metals. H is not part of it.
2. Alkaline earth metals
3. Halogens
4. Noble gasses

Question 22

1. What does the heavy zig zag line separate?
2. Which element is the exception to this rule?
3. All metals are ………. at room temp except for ……… .
4. except for …………. all the elements along the heavy line are ………….. .

Answer 22

1. Metals (to the left) and non-metals (to the right)
2. H. It is not a metal
3. solid, Hg mercury which is liquid
4. aluminum, metalloids

Question 23

1. What is the atomic number?
2. Where does it appear?
3. What charge to atoms have?
4. What is the weighted atomic mass, where is it located on the periodic table?

Answer 23

1. the number of protons an atom has (consequently this also equals the number of electrons).
2. appears above the symbol of the element
3. atoms have a neutral charge (no charge).
4. the weighted average of all naturally occurring isotopes. It is the total number of protons + neutrons. Located under the element.

Question 24

1. what is an isotope?

2. What is an atomic symbol?

Answer 24

1. atoms of the same element, same atomic number, but differing numbers of neutrons.
2. a written way to distinguish between different isotopes

Question 25

How do we calculate atomic mass?

Answer 25

we multiply the mass of each isotope by its abundance and add them all together.

Question 26

1. an electron can change from one energy level to a higher energy level only if it .............. 2. what does an electron do when it moves to a lower energy level?

Answer 26

1. absorbs the energy equal to the difference in energy levels. 2. it emits energy equal to the difference between the two levels.

Question 27

1. does atomic size increase or decrease when working across a period from L-R? Why? 2. does atomic size increase or decrease when working from top of a group downward? Why? 3. in general, ionization energy is ..... for metals and ....... for non-metals. 4. What is ionization energy?

Answer 27

1. atomic size decreases because ionization energy increases, pulling atom in tighter. 2. atomic size increases because ionization energy decreases going down a group. 3. low, high 4. Ionization energy is the required energy to remove one of the outermost electrons. It decreases the further away from the nucleus an electron is located.

Question 28

``` How many electrons are in the following periods, or energy levels (n): period 1: period 2: period 3: period 4: ```

Answer 28

``` n1 = 2 n2= 8 n3= 18 n4= 32 ```

Question 29

periodic trends: | T or F, the number of valence electrons that an atom has coincides with its group number.

Answer 29

True, for the A groups

Question 30

an element that has a high metallic character .............. valence electrons easily

Answer 30

loses

Question 31

1. How many elements are there? 2. Which occur naturally? 3. Which are synthesized?

Answer 31

1. 118 2. 1-94 3. 95-118

Question 32

Name the Halogens and their group number

Answer 32

Group 7A. F Flourine, Cl Chlorine, Br Bromine, I Iodine, At Astatine

Question 33

1. What are the characteristics of metals? 2. What are characteristics of non-metals? 3. What are characteristics of metaloids?

Answer 33

1. shiny, good conductors of electricity, ductile. 2. not shiny, brittle, poor conductors, good insulators 3. semiconductors and insulators

Question 34

1. What are the 4 elements that make up 96% of our body? | 2. What are the 7 macrominerals our body uses for teeth, bones, nerve impulses ect.?

Answer 34

1. Oxygen O, Carbon C, Hydrogen H, Nitrogen N. | 2. Ca, P, K, Cl, S, Na, and Mg

Question 35

What is Dalton's atomic theory?

Answer 35

1. atoms are tiny particles of matter. 2. atoms of an element are similar to each other and different from those of other elements. 3. atoms form compounds and rearrange themselves to form new combinations in a chemical reaction 4. atoms are never created nor destroyed in a chemical reaction

Question 36

what is the mass of a proton, neutron, and electron

Answer 36

proton 1.007 amu neutron 1.008 amu electron 0.000549 amu

Question 37

1. What is electromagnetic radiation? 2. the distance between the peaks of waves is called? 3. high energy radiation has ......... wavelengths, whereas low energy radiation has ......... wavelengths.

Answer 37

1. energy particles that move in waves of energy 2. wavelength 3. short, long.

Question 38

what is an atomic spectrum?

Answer 38

when light from a heated element passes through a prism, it gives off its own unique spectrum of light called "atomic spectrum".

Question 39

what does a Lewis Structure (electron dot symbol) represent?

Answer 39

the number of valence electrons an Element has (this number coincides with the group number for groups 1A to 8A).

Question 40

1. Elements with atomic numbers 20 and higher usually have ................... . 2. An unstable nucleus is .............., emitting small particles of energy called ............... to become more stable. 3. What are the 4 forms of radiation? 4. An isotope of an element that emits radiation is called a ........... ? 5. What happens to the atom when a radioisotope emits radiation?

Answer 40

1. one or more isotopes with unstable nuclei. 2. radioactive, radiation 3. alpha α particles, beta β particles, positrons β+, and pure energy such as gamma γ rays 4. radioisotope 5. it can undergo a change in the number of protons becoming a different element

Question 41

1. What is a geiger counter? 2. what are the appropriate protections for the various types of radiation? 3. Name 4 units for measuring radiation. 4. What is REM? 5. What is the LD50 of radiation for humans?

Answer 41

1. a device to detect beta and gamma radiation. 2. alpha particles = normal clothes or paper. beta particles = heavier clothes. Gamma rays = lead shield, concrete wall, and water. 3. curie, becquerel, rad, and gray 4. radiation equivalent in humans. It measure the biological effects of various types of radiation. 5. 500 rem. 600 rem would be lethal to all humans within a few weeks.

Question 42

1. What is a half life? | 2. How to figure out the half life?

Answer 42

1. The half-life of a radioisotope is the time for the radiation level to decrease (decay) to one-half of the original value. 2. determine the half life of substance. Next divide the time in question by the half life time. Now you know how many half lives you must account for. Now take the mass ie: 36mg and divide by 2. Then divide the answer by 2. Continue dividing the answer by 2 until you have passed the needed number of half lives.