Unit 2 Exam

please don't use only this to study go practice ur math calculations and notations and stuff

metals

the red parts are..

metalloids

the yellow parts are..

non-metals

the blue parts are…

groups

elements in the same ____ have similar chemical properties

Group 1

What group(s) is Alkali metals?

Groups 3-12

What group(s) is transition metals?

Group 18

What group(s) is noble gases?

Group 17

What group(s) is halogens?

57-70

what elements by atomic number are Lanthanides?

89-102

what elements by atomic number are Actinides?

Lanthanides and Actinides

The two types of Transition metals

atom

the smallest particle of an element that retains the properties of that element

electron, proton, neutron

the three smaller parts that atoms are split into

In the electron cloud orbiting the nucleus

Where are electrons?

inside the nucleus

where are protons and neutrons?

The nucleus / protons + neutrons

What makes up the majority of the mass of an atom?

proton

the positively charged subatomic particle of an atom

electron

the negatively charged subatomic particle of an atom

neutron

the subatomic particle of an atom with a 0 charge

Democritus

proposed that everything was made of tiny, indivisible particles called atomos

John Dalton

discovered that different elements were made of different types of atoms; atoms cannot be created or destroyed; all atoms of one type of element are the same

JJ Thompson

Discovered the electron; electrons are negative and protons are positive; believed that protons and electrons were mixed together throughout the atom

Ernest Rutherford

Gold foil experiment; the negatively charged electrons surround the positively charged nucleus of the atom

Niels Bohr

Electrons orbit the nucleus at fixed energy levels; sometimes referred to as the “planetary model”

Werner Heisenberg

cannot pinpoint the exact location of electrons around the atom. Electrons exist in general areas instead.

Atomic Theory

the scientific theory that matter is composed of particles called atoms

Isotopes

Atoms of the same element that the same numbers of electrons and protons but different numbers of neutrons

always stay the same

In isotopes, Atomic number will….

top

in Nuclear Symbol notation, mass goes on the _____

bottom

in Nuclear Symbol notation, atomic number goes on the _____

Hyphen notation

name or symbol of element followed by mass number

Isotopes having different masses

Why are atomic masses on the periodic table not whole numbers?

mole

a counting unit used to describe a very specific number of particles

6.02 × 10^23

Avogadro’s number

Molar mass

moles in a substance related to mass; the mass of one mole of an element

electromagnetic radiation

energy that travels and spreads out as it goes

how atoms emit light

excited electrons fall back from an excited state to a ground state and emits a photon

electromagnetic spectrum

a continuum of all the electromagnetic waves arranged according to frequency and wavelength

increases; frequency

in wavelengths, as energy ___ so does ____

gamma rays, x rays, ultraviolet

wavelengths that are smaller than visible light (in order of smallest to largest)

radio waves, microwaves, infrared

wavelengths that are larger than visible light (in order of largest to smallest)

electrons in the elements differ

why do different elements emit different color light?

spherical

shape of s orbital

dumbbell

shape of p orbital

cloverleaf

shape of d orbital

flower

shape of f orbital

within each subshell, 2 at a time, with opposite spins

where are the electrons in orbitals?

Aufbau principle

electrons fill the lowest energy orbitals first; orbitals within a sublevel have equal energies; for a given main energy level , s < p < d in levels of terms of energy

Pauli Exclusion principle

each orbital can hold 2 electrons with opposite spins; no two electrons can have the same four quantum numbers

Hund’s rule

Within a sublevel, place one e- per orbital before pairing them, all electrons in singly occupied orbitals must have the same spin

2e-

needed total number of electrons to fully occupy n=1

8e-

needed total number of electrons to fully occupy n=2

18e-

needed total number of electrons to fully occupy n=3

32e-

needed total number of electrons to fully occupy n=4

orbital notation

orbitals are represented as boxes; name of orbital written below the line or box; shows spin

full electron configuration

number of electrons in each sublevel show as the superscript; sum of superscript = total number of electrons

noble gas configuration

shows the outermost electrons; writes name of previous noble gas in brackets before completing notation

electrons fill the lowest energy orbitals first

Why do electron configurations for some elements differ