units 2-6 test

Question 1

what is a quanta?

Answer 1

the minimum amount of energy that can be gained or lost by an atom

Question 2

What is a mole?

Answer 2

a mole is an si unit of measuring quantity

Question 3

Where are metals, nonmetals, metalloids (semi-metals), transition metals, inner
transition metals?;

Answer 3

metalloids are any elements touching the stairstep (except aluminum), metals are any element to the left of the metalloids, nonmetals are found in the top right of periodic table, transition metals group 3-12 (3B-12B), inner transition metals are the 2 rows found below the periodic table

Question 4

What types of energy do electrons absorb and emit?; what is the ground state; what is
the excited state; which is more stable?

Answer 4

the ground state is the lowest possible state of an electron; an excited state is anything above that; the ground state is more stable

Question 5

where are halogens

Answer 5

group 17 (7A)

Question 6

what is first ionization energy and what is its trend

Answer 6

the amount of energy required to remove the outermost electron; it decreases from top to bottom and increases from left to right

Question 7

Fusion; uses

Answer 7

fusion is when 2+ small nuclei are forced to combine together to form a bigger nucleus and a huge amount of energy; uses are fusion reactors and the sun

Question 8

Fission; explanation; uses; abuses;

Answer 8

fission is the breaking down into smaller, more stable nuclei; uses are nuclear power plants; abuses are nuclear bombs

Question 9

what is radiation

Answer 9

the penetrating rays and particles given off by a radioactive source

Question 10

where are transition metals

Answer 10

groups 3-12 (3b-12b)

Question 11

How can mass be used to count things?; How can we count atoms and molecules

Answer 11

mass can be used to count things like moles, atoms or representative particles; 6.02*10^25

Question 12

where are noble gases

Answer 12

group 18 (8A)

Question 13

What is Bohr’s Model of the atom

Answer 13

it explained why the atomic emission spectrum for hydrogen only had certain wavelengths of light

Question 14

wavelength

Answer 14

distance between the crests

Question 15

how was nuclear chem discovered

Answer 15

becquerel placed a sample of uranium salts down and saw ti was spontaneously giving off energy. then the curies showed that rays emitted by uranium atoms were causing fogging and named this process radioactivity

Question 16

How are the levels and sublevels arranged?;

Answer 16

energy levels are depicted by a number, sublevels are depicted by a letter

Question 17

what is the most reactive metal and why

Answer 17

the most reactive metals are at the bottoms and to the left
- metals want to lose electrons
-first ionization energy governs losing electrons
-first ie decreases down a group and increases across a period

Question 18

What are Periods? ; groups?;

Answer 18

periods are rows labeled 1-7; groups are columns labeled 1-18 or 1a-8a

Question 19

what is electronegativity and what is its trend

Answer 19

the ability of an atom of an element to attract electrons when the atom is in a compound; it decreases from top to bottom within a group and increases from left to right across a period

Question 20

where are alkali metals

Answer 20

group 1 (1a)

Question 21

frequency

Answer 21

the number of wave cycles to pass at a given point

Question 22

how do different types of light differ?

Answer 22

electromagnetic radiation is energy that moves through space like a wave; atomic emission spectrum is the set of frequencies of the electromagnetic waves emitted by atoms of that element; photoelectric effect is when electrons are emitted from the surface of a metal’s when light of a certain frequency or higher shines on the surface

Question 23

ampiltude

Answer 23

the waves height from zero to crest

Question 24

Atomic emission spectrum;
▪ what is it; how can it be used?

Answer 24

it/s the set of frequencies of the electromagnetic waves emitted by atoms of that element

Question 25

Why isn’t Bohr’s theory thought to be totally correct?; What about the theory is still
accepted?;

Answer 25

some problems were it didnt explain how multiple electrons wouldn’t arrange themselves w/in the energy levels or whther or not you could have more than one electron in an energy level. the part that was accepted was the energy levels

Question 26

Why is it called periodic?; give examples;

Answer 26

because there’s a periodic repetition of their physical and chemical properties

Question 27

What are the major types of nuclear radiation and how can they be distinguished?

Answer 27

alpha loses 2 protons and 2 neutrons; beta converts to a protons and an electron; gamma converts tiny amounts of mass to energy

Question 28

what is the most reactive nonmetal and why

Answer 28

the most reactive nonmetals are at the top and to the right
-nonmetals want to lose electrons
-electronegativity governs gaining electrons
-electronegativity decreases as you go down and increases as you go right

Question 29

● Half-life; what is it?; how can you determine a radioisotopes half-life?; how can it be used to
determine how old a sample is?

Answer 29

the amount of time it takes a one half of a sample of radioisotopes to decay; ex: 20 g of Sr-90 w/1.25 g of Sr-90. How much time? 20->10->5->2.5->1.25=116 years

Question 30

What are the diatomic elements and why are they called diatomic?

Answer 30

h2 n2 o2 f2 cl2 br2 i2 (have no fear of iced cold beer)

Question 31

Evidence of the particle/packet nature of light;

Answer 31

light isn’t a pure wave of energy, it’s a beam of bundles of energy called photons

Question 32

How are electron orbitals depicted and why?;

Answer 32

circular orbitals of defined energy

Question 33

where are alkaline earth metals

Answer 33

group 2 (2A)

Question 34

what is meant by ‘molar mass’?;

Answer 34

it’s the mass of one mol of a specific element (measured in grams)

Question 35

What are some properties of metals, nonmetals and metalloids?

Answer 35

metals are good conductors, high luster, ductility, malleability, and tend to lose electrons in chemical reactions; nonmetals are bad conductors, mostly gases at room temp, and tend to gain electrons in chemical reactions; metalloids’ properties can be affected by the conditions it’s exposed to

Question 36

What are some of the periodic table’s uses?;

Answer 36

it shows the info about the structure of the element’s atoms, shows whether elements are metals, nonmetals, or metalloids

Question 37

what is atomic radius and what is its trend

Answer 37

it’s one half of the distance between the nuclei of 2 atoms and the same elements when the atoms are joined; it increases from top to bottom within a group and decreases from left to right across a period