Unit 3 Chem Periodic Table Test

periodic table

a tool to help u learn about the elements

by the 1860s there were __ elements know

60

how did mendeleeve (russian chem teacher) arrange his table

he arranged them according to their atomic mass

why couldnt mendeleeve arrange the table based off their atomic number

bc it wasnt a thing at the time

today the periodic table is arrangd by the elements __________ __________

atomic number

periodic law

if u arrange elements by increasing their atomic number, trends exsist

4 things in each square

name, symbol, atomic mass, atomic number

optional things in the square

density and electron configuration

periods and what they tell us

horizontal rows, tell us the number of electrons used

groups and what they tell us

vertical groups, tells us number of valence electrons

akali metal

group 1

akali earth metal

group 2

halogens

group 17

noble gases

group 18

number of valence electrons in groups 3-12

undefined

how many valence electrons does He have

2, even tho its a noble gas

where is the s block

left side

where is the d block

in the middle (groups 3-12)

where is the p block

right side

where is the f block

below the rest of the table

element names from latin

au, ag, pb

element names from places

cf, pu, in

element names from people

cm, es, no

elements 1-92 are ________

natural, found on earth

elements 93+ are _________

manmade

rules for symbols of elements

first letter is always capatalized, second is never

characteristics of metals

good conductors, ductile, shiny, malleable

characterastics of semi metals

semi good conductors, semi ductile, semi shiny, semi malleable

characteristics of nonmetals

not good conductors, not ductile, not shiny, not malleable

do noble gases react?

no

why is it called atomic radius

atoms are so small so its hard to see the nucleus

atomic radius _________ as you go down a group, why?

increases bc ur adding electron levels

atomic radius _________ as you go across a period, why?

decreases, more pull from protons in nucleus

what does this metal ion do to become an ion

loose electrons

t or f: a metal ion is smaller than its original ion

true

whst does the nonmetal ion do to become an ion

gains electrons

t or f: a nonmetal ion is smaller than its original ion

false, larger

density ________ as u go down a group, why?

increases, bc the mass is increasing

there is ____ trend for density across a period

no

ionization energy

the energy needed to remove an electron

ionization energy _________ as u go down a group, why?

decreases, bc its further from bullseye

what does the "bullseye" represent for the ionization trend

where the ionization energy is the highest

ionization energy ______ as u go across a period, why?

increases, gets closer to "bullseye"

all elements 92+ are ___________ and ____________

radioactive n unstable

since 92+ elements are radioactive and unstable, the nucleus __________ _________ and __________

breaks apart and decays

why do these 92+ elements decay

too many protons, wont stay together

________ is an isotope of ________, used to date things, this is the exception to the 92+ rule

c-14, carbon

solubility

refers to how things dissolve

solubility __________ as u go across a group, why

decreases, bc elements get heavier

there is ___ trend for solubility across a period

no

why do elements in the same group react the same

same number of valence eletrons

the _______ elements are in a group, the more _______ they are

closer, alike

why should u be conscious of nonmetals, metals, and semimetals in the same group

bc the characteristics are different

most elements are______ at room temp

solid

_____ and _____ are the only elements that are liquids at room temp

hg and br

the rest are ____ at room temp

gases