Semester Midterm- Review

Semester Final- Review- chem

The Comprehensive guide to everything you need to get a 100

Multiple Select

Choose all the qualitative observations.

• The sky is blue

• The jar has 32 marbles

• Bubbles form during a reaction

• An object moves at 12 m/s

Scientific Method

• 1-Observe

• -qualitative- senses

• -quantitative- numbers taken

Multiple Select

What are the PPE we use in the lab?

• Safety Glasses

• Gloves

• Aprons

• Beakers

Scientific Method

• Hypothesis is written in and If(independent), then(dependent), Because(reasoning).

• inDependent is whats changing

• dependent is what is observed quantitatively

• Reasoning is what you think the scientific reason is

• Control- unchanging part of the experiment, vinegar in the baking soda lab

Scientific Method

• 3- Test

• 4-Analyze

• 5-Publish

Multiple Select

Choose the base units

• grams

• decagrams

• m/s

• m

• sec

SI Base units

• grams

• meters

• seconds

• liters

Multiple Choice

An atom is the smallest unit of an element that maintains physical and chemical properties

• True

• False

Atoms

• An atom is the smallest unit of an element that maintains properties

• electron behavior, and intermolecular forces contribute to properties but do not hold properties themselves

Laws of Conservation

• Energy cannot be created or destroyed

• Matter cannot be created or destroyed

• 
  

• 
  

Multiple Select

Choose the older names of Sodium, Copper and, Gold

• natrium

• Ferrum

• cuprum

• argentum

• aurum

Periodic Table

• Many elements have older names

• Copper- cuprum

• Silver-argentum

• Gold- aurum

• potassium- kalium

• sodium- natrium

Multiple Select

What two elements would be most similar?

• F

• Be

• Br

• Cl

• N

Periodic table

• 7 periods, 18 groups, 4 blocks- s, p, d, f

• alkali metals, alkaline earth metals, transition metals, halogens, noble gases, lanthanide and actinide series

• atomic radii increases to the left of a period and down a groups

• electronegativity increases to the right of a period

Multiple Choice

If a metal is soft, silvery, and extremely reactive what group would it belong too?

• transition metals

• alkali metals

• alkaline earth metals

• lanthanide series

Group properties

• Lanthanide series was so similar that originally they could not be separated.

• Actinide series is completely radioactive and all of them are synthetic.

• Alkali metals- soft and silvery, extremely reactive, cannot be found in a pure form in nature

• Alkaline earth metals- less reactive than alkali metals. Higher melting points than alkali metals. Harder and Denser than alkali metals.Still not found in a pure form in nature

• Transition metals- typical metallic properties. Good conductor, high luster, less reactive than alkali and alkaline- earth metals. Some are extremely unreactive, to the point they can be found in pure forms.

• Halogens- Most reactive nonmetals. React with most metals to form salts. Most reactive with alkali metals

Multiple Choice

What element is most electronegative?

• F

• He

• H

• Rn

Periodic Table Trends

• Atomic radii- one-half the distance between the nuclei of identical atoms that are bonded.

  Electronegativity- a measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound

• Ion- atom or group of bonded atoms that has a positive or negative charge

• Ionization- process that results in the formation of an ion.

• Cation- positive charge- metals normally form these

• Anion-negative charge- nonmetals generally form these

Table Trends continued

• Valence electron- electrons available to be lost, gained, or shared in the formation of chemical compounds

• Electronegativity- a measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound

• 
  

• 
  

• 
  

• 
  

• 
  

Multiple Choice

What element is most electronegative?

• F

• He

• H

• Rn

Multiple Select

Choose the properties that are common to metals

• malleable

• liquid at room temp

• goog conductors

• ductile

• brittle

Metals

• metallic bonding- bonding resulting from metal atoms and the sea of electrons( empty orbitals overlap and the valence electrons move constantly through the empty overlapping orbitals)- properties: malleability, conductivity, ductility, high melting points.

• Cations

• malleable

• ductile

• high melting points

• good conductors

Nonmetals

• anion

• Poor Conductors

• Brittle as solids

• Noble gases are highly unreactive

• 
  

• 
  

Metalloids

• All are solids at room temp

• some characteristics of both metals and nonmetals

• 
  

• 
  

Multiple Select

Which of the following of Dalton's Postulates have been disproven?

• atoms cannot be subdivided

• matter is composed of extremely small components called atom

• atoms of an element are all identical in size, mass, and properties

• in chemical reactions, atoms are combined, separated, or rearranged

Dalton's Postulates

• all matter is composed of extremely small particles called atoms

• Atoms of an element are identical in size, mass, and other properties(disproven). Atoms of different elements differ in size, mass, and other properties.

• Atoms cannot be subdivided(disproven), created, or destroyed.

• Atoms of different elements combine in simple whole number ratios to form chemical compounds(law of multiple proportions)

• In chemical reactions, atoms are combined, separated, or rearranged.

Multiple Choice

Which scientist performed the oil drop experiment and discovered the mass of an electron?

• Millikan

• Rutherford

• Thomson

• Bohr

Scientists

• JJ Thomson- theorized the electron- Cathode ray experiment- Plum Pudding Model

• Millikan- Oil Drop experiment- discovered mass of an electron-

• Rutherford- Gold foil experiment- atom is mosty empty space with a dense positive nucleus- Rutherford model

• Bohr- Line emissions spectrum- electrons emit photons of energy that correlate to the light spectrum- Bohr model

• Mendeleev- arranged the periodic table by properties and guessed three elements correctly- discovered periodicity

• Moseley- arranged periodic table by atomic number and properties

Multiple Select

What does a nucleus of an atom hold?

• protons

• electrons

• molecules

• neutrons

atoms, types, and subatomic particles

• a neutral atom is what we find on the periodic table. atomic number=protons=electrons

• neutrons= mass-atomic number

• a isotope has a mass other than that on the periodic table- C-12, C-14

• an ion holds a charge meaning electrons have been either lost or gained

Multiple Select

Choose the electromagnetic radiation types.

• Light spectrum

• radio waves

• UV light

• infrared

• Gamma

Electromagnetic radiation, waves, and electron behavior

Multiple Choice

What light has the highest frequency?

• violet

• red

• blue

• green

Multiple Choice

What light has the shortest wavelength?

• violet

• red

• blue

• green

Multiple Choice

How many moles are in 12 g of C2O2?

• .21 mol

• .43 mol

• 4.7 mol

• 2.3 mol

Multiple Choice

How many particles are in 12 g of C2O2?

• 1.26

• 1.26x10²³

• 2.52x10²³

• 1.52

Mole conversions

• Avogadro’s number= 6.02x10^23= 1 mol

• 22.4 L of a gas at STP= 1 mol

• Molar mass of an element= 1 mol

  
  

Multiple Choice

What is the noble gas configuration of neutral Se?

• [Ar]4s²3d¹⁰4p⁴

• [Ar]4s²4d¹⁰4p⁶

• [Ar]4s²3d¹⁰4p6

Electron Configurations

• 3 ways to indicate configuration of electrons

• Electron configuration- 1s²2s²2p⁶3s²....

• Orbital notation is when we draw whats above

• Noble gas configuration is using our noble gases to indicate the configuration up to that point

• 7 energy levels, a new sublevel is introduced in each.s- 1 orbital, p-3 orbitals, d- 5 orbitals, f-7 orbitals. An orbital holds two electrons

• aufbau principle- electrons will occupy the lowest eneryg orbital that will recieve it

• Hund's Rule-orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin state.

quantum numbers

​principle number- energy level

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​angular momentum- sublevel- s,p,d,f

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​magnetic number- orientation- s-1, p-3, d-5, f-7

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​spin- direction of spin- opposite in an orbital

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​​pauli exclusion principle- no two electrons in an atom can have the same set of 4 quantum numbers

Multiple Choice

Ionic bonds do what with electrons?

• share

• gain/lose

Bonds

• Ionic Bond- bond between a cation and an anion- forms a lattice structure- 1.71 and up for electronegativity difference- strongest bond

• Non-Polar Covalent- equal sharing of electrons between two atoms- 0-.3 electronegativity difference- weakest bond

• Polar Covalent -unequal sharing of electrons between atoms- .31-1.70 electronegativity difference

• Molecule- neutral group of atoms held together by covalent bonds

• Molecular compound- compound whose simplest unit is a molecule- low melting points- often liquids or gases.

• Ionic compound- anion and cations arranged in a lattice structure- high electrostatic force- lattice structure is its minimum potential energy- non-conductive when solid but conductive when aqueous(NaCl)

Multiple Choice

Which of these is a formula unit?

• NaCl

• OF₂

• Na₂Cl₂

• SCl₂

Formulas

• Empirical formula: lowest ratio of atoms in a molecule

• Molecular formula: actual number of atoms in a molecule

• Formula unit: ratio of cations to anions

Multiple Select

What 2 elements contradict the octet rule?

• H

• He

• B

• Na

• Octet rule- atoms want to have a full outer shell of valence electrons. Exceptions- Hydrogen only needs to have two electrons. Boron only has 3 available valence electrons to bond. Some atoms can have expanded valence tendencies.

• Multiple Bonds- double or triple bonds formed when multiple electron pairs are needed to be shared to satisfy the octet rule. Carbon often forms these.

• Dipole- a compound that has an offsetting charge throughout itself making it non-neutral. Just because a molecule has polar bonds does not mean that the molecule as a whole is polar. Geometry and electronegativity play huge roles in determining these.

Geometry

• Step:1- FIgure out how many valence electrons there are

• 2- less electronegative atom is central (exception H and C)

• 3- pair of electrons between central atom and each outer atom

• 4- complete octets

• 5- double and triple bonds if needed

• 6- determine form

• 7- determine geometry

Geometry continued

• Geometry-

• AB, AB2- Linear

• AB3- trigonal-planar

• AB4- Tetrahedral

• AB2E, AB2E2- bent

• AB3E- trigonal-pyramidal

• 
  

Intermolecular Forces

• Ion-ion- force resulting from oppositely charged ions being attracted to one another.- individually strongest of the intermolecular forces

• Ion-dipole- force resulting from the partially charged sides of a dipole molecule being attracted to the fully charged ion of an ionic compound- NaCl dissociates in water Na is attracted to the negative oxygen and Cl to the positive hydrogen.

• Dipole-Dipole- force resulting from the oppositely charged ends of a dipole being attracted to one another. 

• Hydrogen bonding- strongest dipole-dipole force, the high positive charge created in the outer hydrogen atoms makes it attracted to highly electronegative atoms lone pairs.

• London dispersion forces- forces constantly acting- weakest of the forces. A momentary dipole is created in an otherwise neutral atom creating an induced dipole of another atom 

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