U7 Atoms and Elements Flashcards

Atom

Basic unit of matter

Parts of an atom

Protons, Neutrons, and Electrons

Charge of a proton

Positive (+)

Charge of a neutron

No charge

Charge of an electron

Negative (-)

Element

Pure substance that consists of entirely one type of atom.

Balanced Element Factors

Same numbers of protons and electrons; number of neutrons according to periodic table.

Parts of Element on Periodic Table

Atomic Number, Element Symbol, Element Name, Atomic Mass

Atomic Mass

Number of protons and neutrons in element

Atomic Number = ?

Protons and Electrons

Electrons in a neutral atom = ?

Protons and Atomic Number

Neutrons = ?

Atomic mass - atomic number

Mass of Protons

1 g

Mass of Electrons

0.00001 g

Mass of Neutrons

1 g

Ions

An atom with a different number of electrons

Isotope

An atom with a different number of neutrons

Cations

Positively Charged

Cations [blank] electrons

Lose

Anions

Negatively Charged

Anions [blank] electrons

Gain

Polyatomic Ions

Ions that have more than one atom

Radioactive Isotopes

Isotopes with an unstable nucleus and give off alpha, beta, and gamma energy.

Atom with a different number of protons

Some element; depends on the number of protons

Aluminum ion

Al³⁺

Copper ion

Cu⁺ or Cu²⁺

Calcium ion

Ca²⁺

Iron ion

Fe⁺²  or  Fe⁺³

Sodium Ion

Na⁺¹

Tin

Sn⁺²  or  Sn⁺⁴

Zinc

Zn⁺²

Ammonium

NH₄⁺¹

Carbonate

CO₃^-2

Chloride or Chlorine

Cl^-1

Hydroxide

OH^-1

Nitrate

NO₃^-1

Nitrite

NO₂^-1

Nitride or Nitrogen

N^-3

Oxide or Oxygen

O^-2

Phosphate

PO₄^-3

Sulfate

SO₄^-2   

Chlorate

ClO₃^-1

Chromate

CrO₄^2-

John Newlands

Arranged elements according to their atomic mass and chemical properties

Law of Octaves

Properties repeat every 8 elements

Dmitri Mendeleev

Organized elements by increasing atomic mass and sorted them in new rows for chemical properties; left missing spots in the table

Henry Moseley

Reorganized table into increasing atomic number and made sense; realized wavelengths related to atomic number not mass

Groups/family

Each vertical column in the periodic table

Properties of elements in the same family

Valence electrons, charges as an ion, and physical and chemical properties

Periods

Horizontal rows of the periodic table

Properties of elements in the same period

Same electron configuration and energy level

Synthetic Elements

Man-made elements

Alkali Metals

Group 1; One valence electron; +1 Ion charge

Alkaline-Earth Metals

Group 2; 2 valence electrons; +2 Ion charge

Halogens

Group 17; 7 valence electrons; -1 Ion Charge

Noble Gases

Group 18; 8 valence electrons; stable and unreactive

Metals

Shiny, good conductor of electricity, malleable, ductile

Nonmetal

Dull, brittle, not malleable, poor conductor of electricity

Metalloids

Mix of metal and nonmetal characteristics

Atomic mass

Atomic mass units (amu); number of protons and neutrons

JJ Thomson

Discovered the electron was negatively charged in 1897 and proposed Plum Pudding Model

Plum Pudding Model

Cloud of positive charges with negative electrons evenly mixed in

Gold Foil Experiment

Experiment done to prove the validity of the Planetary Model of an atom

Planetary model

Protons and neutrons in center of atom and electrons on outside.

Findings of gold foil experiment

If alpha particles pass straight through gold foil = atoms made of mostly open space; bouncing back = hit positively charged part of atom (i.e. protons)

Bohr’s Atom Model

Based on the assumption that electrons travel in specific shells, or orbits, around the nucleus

Valence Electrons

Electrons on the outermost ring of an atom (based on Bohr’s Atom Model)

Orbitals

Regions around nucleus where electrons most likely to be found

Types of orbitals; orbital shapes

S, P, D, F

Shells of electron configuration

1, 2, 3…

Pauli Exclusion Principle

Only two electrons can occupy one orbital at the same time

Shell notation of orbital configuration; Quantum Number

1s, 2s, 3s…

Aufbau Principle

Fill electrons from lowest energies first (1, 2, 3,..)