The force that holds atoms or ions together as a unit.

The amount of energy used to remove an electron. The lower the ionization, the easier it is to remove an electron from an atom.

Trends for ionization energy

Ionization energies tend to increase from left to right across a period. Ionization energies tend to decrease from the top of a group to the bottom.

The number of electrons an atom needs to lose or gain to become stable.

A notation that shows what elements a compound contains and the ratio of the atoms or ions of these elements in the compound.

Solids whose particles are arranged in a lattice structure.

Properties of an ionic compound

High melting points, poor conductor of electricity as a solid, good conductor of electricity as a liquid, shatters when hammered.

Reason for properties of ionic compounds

Ionic compounds have strong electrostatic forces between ions, which contribute to their high melting points and brittleness.

A chemical bond in which two atoms share one pair of valence electrons.

A neutral group of atoms that are joined together by one or more covalent bonds.

Covalent bonds held together by

Attractions between the shared electrons and the protons in each nucleus hold the atoms together.

Subscript in a formula

How many atoms of each element are in the formula.

2 atoms of the same element. Many non-metals exist as diatomic molecules. Ex: H₂

When two atoms share two pairs of electrons. Ex: O₂

When two atoms share three pairs of electrons. Ex: N₂

Polar covalent bond definition

A covalent bond in which electrons are not shared equally.

Partial negative charge in polar covalent bond

The atom with the greater attraction for electrons has a partial negative charge.

Factors determining if a molecule is polar or nonpolar

Type of atoms in a molecule and its shape.

It has single bonds and the bonds are polar because oxygen has a greater attraction for electrons. Also, since the molecule has a bent shape, the polar bonds do not cancel each other out.

Carbon dioxide's nonpolarity

CO₂ has double bonds and each double bond is polar. But, since it is linear, the double bonds pull on each other and the pull cancels out, making the whole molecule nonpolar.

Attraction strength comparison

Polar has stronger attractions.

Naming a binary ionic compound

A binary ionic compound is named by combining the name of the cation (metal) and the name of the anion (nonmetal) with the anion's name ending in -ide.

Name of cation (metal) first, root name of anion (nonmetal) second, suffix -ide used on anion.

Naming convention for ionic compounds.

The name of the metal is first with the Roman numeral to indicate the charge on the ion in parenthesis.

How a metal with multiple ions is named.

A covalently bonded group of atoms that has a positive or negative charge and acts as a unit.

Definition of a polyatomic ion.

Symbol of cation first, followed by symbol of anion. Subscripts show the ratio of ions in the compounds.

How the formula for an ionic compound is written.

The total charges of the cations and anions must add up to zero.

How ionic compounds become neutral.

Subscript representation in an ionic formula

Indicates how many atoms of each element are in the formula.

Naming a molecular (or covalent) compound

1) The most metallic element appears first. 2) The second element ends with the suffix -ide. Example: Nitrogen oxide and diphosphorus trioxide.

Writing a molecular (or covalent) formula

1) Write the symbols for the elements in the order they appear in the name. Prefixes indicate the number of atoms of each element in the molecule and appear as subscripts in the formulas.

Definition of a metallic bond

Attraction between a metal cation and the shared electrons that surround it.

Good conductors of heat and electricity, malleable and ductile.

Role of lattice structure in metals

The lattice structure allows metals to be flexible, making them malleable and ductile.

Metallic bonds are held together by the cations in a metal forming a lattice held by strong metallic bonds between the cations and the surrounding valence electrons.

The cations in a metal form a lattice held by strong metallic bonds between the cations and the surrounding valence electrons.

An alloy is a mixture of two or more elements, at least one of which is a metal.

A mixture of two or more elements, at least one of which is a metal.

Different types of alloys exist because scientists can design alloys with specific properties by varying the types and amounts of elements in an alloy.

Scientists can design alloys with specific properties by varying the types and amounts of elements in an alloy.

Steel is made from iron and a small amount of carbon.

Iron and a small amount of carbon.

Stainless steel is different because it contains iron and more than 10% by mass of chromium and almost no carbon.

It contains iron and more than 10% by mass of chromium and almost no carbon.

Chemistry Concepts Flashcards

Student preview

47 questions

Show all answers

1.

FLASHCARD QUESTION

Front

Stable electron configuration

Back

The outer energy level is full with 8 valence electrons.

2.

FLASHCARD QUESTION

Front

Electron dot diagram

Back

Model of an atom in which each dot represents a valence electron.

3.

FLASHCARD QUESTION

Front

Element symbol

Back

The symbol in the center represents the nucleus and all the other electrons in the atom.

4.

FLASHCARD QUESTION

Front

Ion formation

Back

When an atom gains or loses electrons, it takes on a charge.

5.

FLASHCARD QUESTION

Front

Ionic bond

Back

An ionic bond is between a metal (cation) and a nonmetal (anion).

6.

FLASHCARD QUESTION

Front

Anion

Back

An ion with a negative charge.

7.

FLASHCARD QUESTION

Front

Cation

Back

An ion with a positive charge.

Access all questions and much more by creating a free account

Create resources

Host any resource

Get auto-graded reports

Continue with Google

Continue with Email

Continue with Classlink

Continue with Clever

or continue with

Microsoft

Apple

Others

Already have an account?

Similar Resources on Wayground

37 questions

Grade 11 CAT

Flashcard

•

11th Grade

35 questions

Motion in Two Dimensions

Flashcard

•

12th Grade

49 questions

REVIEWER FOR PREFINALS in MATHEMATICS 8

Flashcard

•

8th Grade

42 questions

Overview of the Internet and Key Concepts

Flashcard

•

University

44 questions

Spanish Vocabulary Flashcards

Flashcard

•

4th Grade

40 questions

Grammar and Use of English Flashcard

Flashcard

•

Professional Development

36 questions

Pre-Test: Matter Cycling & Photosynthesis

Flashcard

•

7th Grade

46 questions

HGeo Unit 2 Test Review

Flashcard

•

9th Grade - University

Popular Resources on Wayground

15 questions

Fractions on a Number Line

Quiz

•

3rd Grade

20 questions

Equivalent Fractions

Quiz

•

3rd Grade

25 questions

Multiplication Facts

Quiz

•

5th Grade

54 questions

Analyzing Line Graphs & Tables

Quiz

•

4th Grade

$fractions$

22 questions

fractions

Quiz

•

3rd Grade

20 questions

Main Idea and Details

Quiz

•

5th Grade

20 questions

Context Clues

Quiz

•

6th Grade

15 questions

Equivalent Fractions

Quiz

•

4th Grade

Discover more resources for Science

10 questions

Butterfly Life Cycle

Quiz

•

KG