Exam 1

Question 1

components in an atom

Answer 1

electrons, protons, and neutrons

Question 2

how to convert step by step

Answer 2

1. start with the known
2. use conversion factor
3. denominator should cancel out
4. multiply all numerators
5. divide by denominators
6. final answer

Question 3

symbol z with dash means?

what does it defines and represent?

Answer 3

for atomic number.
defines atom identity
represents number of protons

Question 4

mass number located where?

Answer 4

at the bottom of the element on periodic table but flipped elsewhere

Question 5

natural abundance where to find it?

Answer 5

i dont know

Question 6

isotopes def

Answer 6

atoms with same number of protons but different neutrons

Question 7

how to find neutrons?

Answer 7

mass number -proton number

Question 8

electrons are found?

Answer 8

number of protons - what will give the number of electrons charge indicates

Question 9

main group elements?

Answer 9

representative elements; groups with A behind

Question 10

bon-rep elements

Answer 10

transition and inner tradition metals; groups w/ B

Question 11

groups equals ?

periods equals ?

Answer 11

columns

rows

Question 12

Alkali metals are where?
Alkaline earth metals?
Halogens?
Noble has?
is hydrogen a alkali metal?

Answer 12

Column 1 
Column 2
Column 17
Column 18
non-metal

Question 13

ionic compounds def
which compounds are ionic?
def of ion?
difference between cation and anion?

Answer 13

comprised of ions that are held together by electrostatic attraction
formed between a metal and non mental 
cation positively charged ion
anion negatively charged ion
ion is an electrically charged species

Question 14

salt def

Answer 14

any cation or anion pair

Question 15

molecular mass def?

Answer 15

mass of all the atoms

Question 16

mile number; and name of creator

Answer 16

6.02x10^23; Avogadro

Question 17

When using mole equation what is the overall end? what do you do last?

Answer 17

multiply numerators by denominators

Question 18

describe step by step how to do a mol conversion

Answer 18

1. start with given
2. find the element amu in grams to cross out and put one mom on top
3. put one mil of given on bottom to cross out and put mol of wanted on top
4. put mol of wanted on bottom and amu of wanted on top.
5. multiply all on top and divide by bottom

Question 19

wavelength symbol is?

Answer 19

lambda

Question 20

nu is? how to calculate?

Answer 20

frequency; 1/seconds

Question 21

speed of light equation?

Answer 21

c=(lambda)(nu)

Question 22

frequency increase and energy does what?

Answer 22

increase

Question 23

trident equals what?
trident is what?
trident squared means what?

Answer 23

how much energy in electron
psi
where the electron is

Question 24

quantum numbers are for what?

what is principle quantum number?

Answer 24

describe an electron
n
can be 1,2,3….

Question 25

l = | what’s its limits and give example

Answer 25

l = angular momentum quantum number limited by the value n n=2 n=3 n=3

Question 26

L does what?

Answer 26

determine shape of volume of space where electron is; the orbital

Question 27

what does 0,1,2,3 equal?

Answer 27

s, p, d, f

Question 28

mL is? | in comparison to the orbitals

Answer 28

orientation in 3D space s (L=0 ml=0) one s orbital p (L=1 ml=-1,0+1) three p orbitals d (L=2 ml = -2,-1,0,+1,+2) five d orbitals so third shell has one s, 3p and 5d orbitals

Question 29

ms = ? represents what? number quantity

Answer 29

electron spin quantum number represent the up and down arrows 1/2 or -1/2. depends on the arrow

Question 30

orbital is what?

Answer 30

the volume of space in which an electron is likely to be found

Question 31

s orbitals are shaped? | p?

Answer 31

spherical | dumbbell

Question 32

pauli exclusion principle

Answer 32

implies that an individual orbital defined by n, l, ml values can hold a max of two electrons (one with ms +1/2 and one with ms -1/2)

Question 33

aufubau principle

Answer 33

start with ground state and build up always filling +1/2 first and then adding -1/2.

Question 34

hunds rule

Answer 34

the most stable arrangement of electrons is the one with the greater number of parallel spins. so singly fill up before down.

Question 35

valence electrons

Answer 35

electrons in the outer shell

Question 36

what is common about halogens F, Cl, Br, and I?

Answer 36

they all have seven valence electrons

Question 37

how to calculate valence electrons by looking at periodic table?

Answer 37

group 1 - 1 valence | group 18 - 8 valence

Question 38

excited state?

Answer 38

electron is unstable. in a higher energy orbital than its ground state. will probably fall back and lose energy

Question 39

noble gases explain

Answer 39

are very stable and unreactive | have filled shells and sub shells

Question 40

atomic radii explain

Answer 40

increase going down a column | raid decrease from left to right across row

Question 41

ionic radii

Answer 41

loses an electron to form action so size decreases | gains electron to for anion size increases

Question 42

isoelectronic series

Answer 42

a series of ions they have the same electron configuration

Question 43

electronegativity def

Answer 43

an atoms ability to pull electrons toward itself; increase as u go up a column and from left to right. florine is most EN but noble gases don’t have them because they don’t form bonds and are stable

Question 44

non metals do what in electronegativity ? | metals?

Answer 44

``` nonmetals = bigger metals = smaller ```

Question 45

electronegativity rules of thumb

Answer 45

EN difference of 2.0 or less is an ionic bond EN différence of greater than 2.0 is covalent EN between o.5 and 2.0 polar covalent EN less than 0.5 is bon polar covalent bonds